Search found 102 matches
- Fri Mar 12, 2021 1:58 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Textbook Problem 5.33 Parts A and D
- Replies: 2
- Views: 267
Textbook Problem 5.33 Parts A and D
Hey guys! I'm a little confused on parts A and D of the textbook problem 5.33. -For part A, I don't understand how you can tell the reaction is endothermic. Is this inferred because the reaction takes place at such a high temperature, or is there a concrete way to tell that the given reaction is end...
- Fri Mar 12, 2021 12:39 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equilibrium Constants and Solubility
- Replies: 2
- Views: 293
Equilibrium Constants and Solubility
Hey guys!
One of the bullet points on outline #1 for chemical equilibrium states "use equilibrium constants to predict solubility". Can someone explain the correlation between solubility and the equilibrium constant? Thanks in advance!
One of the bullet points on outline #1 for chemical equilibrium states "use equilibrium constants to predict solubility". Can someone explain the correlation between solubility and the equilibrium constant? Thanks in advance!
- Wed Mar 10, 2021 1:04 am
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Value of N
- Replies: 24
- Views: 1196
Value of N
Hey guys!
I'm having issues figuring out the value of n to use in the NERNST equation. If someone could explain how to get this value, it would be appreciated!
I'm having issues figuring out the value of n to use in the NERNST equation. If someone could explain how to get this value, it would be appreciated!
- Wed Mar 10, 2021 12:29 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Textbook Problem 6M.5 Part B
- Replies: 1
- Views: 126
Textbook Problem 6M.5 Part B
Hey guys! When I was checking my answers for the textbook problem 6M.H, specifically part B, I noticed that the answer key did not include a calculation for ΔG°. I was wondering if this reaction doesn't have a value for ΔG° because the standard cell potential was negative? Or maybe the answer key is...
- Tue Mar 09, 2021 9:16 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing Half Reactions in Acidic/Basic Solution
- Replies: 3
- Views: 343
Re: Balancing Half Reactions in Acidic/Basic Solution
Hi! My approach varies slightly from yours. This is how I have been solving these problems: 1. For acidic and basic solutions, balance atoms other than H and O atoms. 2. For acidic and basic solutions, balance O atoms with H2O. 3. For acidic and basic solutions, use H+ to balance H atoms. (You are ...
- Tue Mar 09, 2021 8:41 pm
- Forum: Balancing Redox Reactions
- Topic: Balancing Half Reactions in Acidic/Basic Solution
- Replies: 3
- Views: 343
Balancing Half Reactions in Acidic/Basic Solution
Hey guys! I just wanted to double check that I am using the correct to approach to balancing half reactions in acidic solution vs basic solution. No matter if the half reaction is in acidic solution or basic solution, the first step is to balance any atoms other than H and O atoms. Once all other at...
- Sat Mar 06, 2021 11:48 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: k'
- Replies: 4
- Views: 272
Re: k'
Hey Trevor! I believe that the difference between k and k' is that k' is calculated using data in which the concentrations of the reactants have been manipulated whereas k is calculated using data in which the concentrations of the reactants are more or less left alone (the concentrations of the rea...
- Sat Mar 06, 2021 11:40 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Molecularity
- Replies: 10
- Views: 469
Re: Molecularity
Hey Ashley! I'm pretty sure that you can look at the stoichiometric coefficients when determining molecularity. In lecture #24, Dr. Lavelle said that the reaction A+A→P is bimolecular. Another way of writing this reaction is 2A→P, and I believe that because the reactions are the same thing (just wri...
- Sat Mar 06, 2021 11:34 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: k'
- Replies: 8
- Views: 610
Re: k'
In a reaction with multiple reactants, k' won't be the same for each reactant. k' appears in the rate law when a reaction has been manipulated to have one reactant in a much lower concentration than the others. Therefor, when you manipulate the concentration of different reactants, k' will be differ...
- Sat Mar 06, 2021 11:27 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Rate Laws and Elementary Steps
- Replies: 4
- Views: 275
Rate Laws and Elementary Steps
Hey guys! I just want to double check and make sure I'm understanding the rate laws of elementary steps correctly. Essentially, all the molecules in elementary steps have to be colliding with one another and are therefor involved in the reaction. Using this information, you can write the rate laws o...
- Sat Mar 06, 2021 11:20 pm
- Forum: Experimental Details
- Topic: Determining Rate Law of a Reaction With Multiple Reactants
- Replies: 2
- Views: 375
Determining Rate Law of a Reaction With Multiple Reactants
Hey guys! In Lecture #24, Dr. Lavelle explained that if you have a reaction with multiple reactants, you can determine the rate of the reaction by making the concentration of one reactant very small compared to the others. I understand this experimental process for finding the rate law, but me quest...
- Sun Feb 28, 2021 3:38 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Direction of ion flow in Galvanic cells
- Replies: 6
- Views: 2603
Re: Direction of ion flow in Galvanic cells
Hey Gabby! In order for Galvanic cells to function, there can't be a buildup of charge on either side of the cell so ions are actually flowing in both directions through the salt bridge or porous disk. Which way they are flowing depends on the positions of the anode and cathode. Anions are going to ...
- Sun Feb 28, 2021 3:31 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: anode / Cathode
- Replies: 9
- Views: 629
Re: anode / Cathode
Would we be more focused on Galvanic cells for this section or do we memorize different how it applies to different cells? I think it would be best to try and remember how both Galvanic and electrolytic cells work and the differences between them. However, in lecture #20, I believe that Dr. Lavelle...
- Sun Feb 28, 2021 3:22 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: What is Potential?
- Replies: 14
- Views: 655
What is Potential?
Hey guys!
I'm a little confused on what exactly potential is. For example, when you say that the cathode has more potential than the anode, what does this mean? Does it have to do with its ability to pull electrons towards itself? Thanks in advance!
I'm a little confused on what exactly potential is. For example, when you say that the cathode has more potential than the anode, what does this mean? Does it have to do with its ability to pull electrons towards itself? Thanks in advance!
- Sun Feb 28, 2021 3:18 am
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: E° vs. E and G° vs. G
- Replies: 25
- Views: 1083
E° vs. E and G° vs. G
Hey guys! I just wanted to clarify the difference between E° vs. E and G° vs. G. E° and G° are the potential and Gibbs free energy, respectively, for the system at standard conditions, and E and G are the potential and Gibbs free energy, respectively, for the system not at standard conditions? Basic...
- Sat Feb 27, 2021 12:07 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Potential Difference
- Replies: 1
- Views: 147
Potential Difference
Hey guys! I'm a little bit confused on part of the content from lecture #17. In this lecture, Dr. Lavelle said that potential differences between electrodes causes electron movement. What exactly does he mean by potential difference? And what would cause an electrode to have more potential than anot...
- Mon Feb 22, 2021 3:07 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Which R Values to use
- Replies: 22
- Views: 8674
Re: Which R Values to use
Hey Danielle! I don't think there is a set situation for which you would use either R value. Instead, which R value you use depends on the units you're dealing with. When R=0.08206, the units are (L.atm)/(K.mol). When R=8.314, the units are (J)/(K.mol). To decide which R value to use in a given situ...
- Mon Feb 22, 2021 3:02 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Calculating degeneracy
- Replies: 18
- Views: 3545
Re: Calculating degeneracy
Hey Anya!
Personally, how I like to calculate degeneracy is with the formula W=x^n where x is the number of positions and n is the number of molecules. For example, if you have a mole of molecules with five possible positions, W=(5)^(6.022x10^23). Hope this helps!
Personally, how I like to calculate degeneracy is with the formula W=x^n where x is the number of positions and n is the number of molecules. For example, if you have a mole of molecules with five possible positions, W=(5)^(6.022x10^23). Hope this helps!
- Mon Feb 22, 2021 2:59 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Exergonic Rxns
- Replies: 14
- Views: 775
Re: Exergonic Rxns
Hey Emily!
I believe that all exergonic reactions are spontaneous because the ΔG of an exergonic reaction is negative. Hope this helps!
I believe that all exergonic reactions are spontaneous because the ΔG of an exergonic reaction is negative. Hope this helps!
- Thu Feb 18, 2021 7:34 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Textbook Problem 4D.7
- Replies: 1
- Views: 157
Textbook Problem 4D.7
Hey guys! I'm having some trouble with question 7 in section 4D. The question reads: "Oxygen difluoride is a colorless, very poisonous gas that reacts rapidly and exothermically with water vapor to produce O2 and HF: OF2(g) + H2O(g) → O2(g) + 2HF(g). ΔH=-318 kJ. What is the change in internal e...
- Thu Feb 18, 2021 5:46 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Textbook Question 4C.3
- Replies: 2
- Views: 187
Textbook Question 4C.3
Hey guys! I'm having some trouble with question 3 in section 4C. The question reads: Calculate the final temperature and the change in enthalpy when 765 J of energy is transferred as heat to 0.820mol Kr(g) at 298 K and 1.00 atm (a) at constant pressure; (b) at constant volume. Treat the gas as ideal...
- Sun Feb 14, 2021 5:30 am
- Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
- Topic: Sapling # 14
- Replies: 6
- Views: 385
Re: Sapling # 14
Hey Alex! You can use the formula ΔS=ΔH/T to solve this problem. Basically, because you are given the ΔS and ΔH for vaporization, you can plug the given values into this equation and solve for T because the temperature of vaporization is boiling point. One note is that you have to make sure that bot...
- Sun Feb 14, 2021 5:19 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Sapling Week 5/6 #18
- Replies: 7
- Views: 422
Re: Sapling Week 5/6 #18
Hey Molly! The inverse of a natural log is e, and you have to use this property to solve for K in this problem. What I did was take the formula ΔG∘r=-RTln(K) and solved for ln(K) first. When I did this, I got ln(K)=(ΔG∘r)/(-RT). Then I used the inverse logarithmic property for natural logs and solve...
- Sun Feb 14, 2021 5:11 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy: kJ or J?
- Replies: 30
- Views: 1658
Re: Entropy: kJ or J?
Hey Raquel! I believe that the most common unit for entropy is going to be J, however it really depends on the problem. One trick to make sure you are making your calculations with the correct units is to look at the units of the answer (which are given to us on both the Sapling problems and on the ...
- Sun Feb 14, 2021 5:08 am
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Sapling #5 week 5 and 6
- Replies: 13
- Views: 674
Re: Sapling #5 week 5 and 6
Hey Hana! Here's a list of the steps I took to solve this problem. 1. Convert the given temperatures from Celsius to Kelvin. 2. Calculate the number of moles present in the beginning of the reaction using the equation PV=nRT. When you solve for n, this equation becomes n=(PV)/(RT). 3. Calculate ΔS u...
- Sun Feb 14, 2021 4:50 am
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Complex Molecules and Entropy [ENDORSED]
- Replies: 1
- Views: 80
Complex Molecules and Entropy [ENDORSED]
Hey guys! In lecture #15, Dr. Lavelle said that complex molecules have more entropy because complex molecules can have a greater number of different orientations for the atoms in the molecule. Given this information, would it be incorrect to say that molecules with resonance would have greater entro...
- Sun Feb 07, 2021 4:15 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: HW Question
- Replies: 4
- Views: 465
Re: HW Question
Hey Brandon! The first thing you need to do to solve this problem is draw the Lewis structure for CO2 and decide wether it is a linear or nonlinear molecule. This will tell you what value to use for heat capacity. Once you've done this, you solve for q using the equation q=mcΔT where m is mass, c is...
- Sun Feb 07, 2021 4:03 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Using R in thermodynamic equations
- Replies: 24
- Views: 1091
Re: Using R in thermodynamic equations
Hey Melody! Basically whatever R value you use depends on what units you're dealing with and what you're trying to solve for. If you want your final answer to be in L.atm, you would use the R value 0.0821 L.atm/K.mol. If you want your final answer to be in , you would use the R value 8.314 J/K.mol. ...
- Sun Feb 07, 2021 3:48 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Sapling #14
- Replies: 6
- Views: 371
Re: Sapling #14
Hey Olivia! For this problem, the first step is to solve for moles using the equation PV=nRT. Basically, you just substitute the given values for P (pressure), V (volume), and T (temperature) and R=0.0821 L*atm/mol*K to solve for n. For the volume, you have to substitute the original volume because ...
- Sun Feb 07, 2021 3:38 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Sapling wk 3/4 #17
- Replies: 5
- Views: 605
Re: Sapling wk 3/4 #17
Hey Melody! For this question, you have to use two equations. The first equation is U=q+w where U is internal energy, q is the energy going in or out of the system, and w is work. Because you are given values for internal energy and work, you can substitute them into the equation and solve for q. On...
- Sun Feb 07, 2021 3:32 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Internal Energy Definition
- Replies: 6
- Views: 259
Internal Energy Definition
Hey guys!
I'm a little confused about what exactly internal energy actually is. If someone could define it or explain what the internal energy of a system is, it would be appreciated. Thanks in advance!
I'm a little confused about what exactly internal energy actually is. If someone could define it or explain what the internal energy of a system is, it would be appreciated. Thanks in advance!
- Sun Jan 31, 2021 6:28 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: How Does Temperature Affect the Equilibrium Constant?
- Replies: 25
- Views: 22708
Re: How Does Temperature Affect the Equilibrium Constant?
Hey Lilyana! Basically, if the reaction is endothermic, then heating will favor product formation and increase K. If the reaction is exothermic, then heating will favor reactant formation and decrease K. I like to think of heat as either a product or a reactant depending on the reaction, and this he...
- Sun Jan 31, 2021 6:18 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Making X negligible
- Replies: 34
- Views: 1484
Re: Making X negligible
Hey Sean! If the problem has a Kc value that is less than 1.0 x 10^-4, you can approximate that the value of X becomes negligible. You can do this because the small Kc value indicates that there is very little product formed at equilibrium, meaning that the concentration of the reactants isn't chang...
- Fri Jan 29, 2021 2:45 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Textbook Problem 4D.23
- Replies: 1
- Views: 101
Textbook Problem 4D.23
Hey guys! I'm kinda confused on how to solve textbook problem 4D.23. For this problem, we are supposed to calculate the standard energy formation of dinitrogen pentoxide using two given equations and their standard reaction enthalpies. 1) 2NO(g) + O2(g) → 2NO2(g) ΔH=-114.1 kJ 2) 4NO2(g) + O2(g) → 2N...
- Thu Jan 28, 2021 8:39 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Textbook Problem 5.61 Part F
- Replies: 2
- Views: 151
Textbook Problem 5.61 Part F
Hey guys! I'm a little confused on textbook problem #5.61, specifically part F. For this problem, we are supposed to predict the effect of a given change on the equilibrium composition of the equation 6CO2(g) + 6H2O(l) → C6H12O6(aq) + 6O2(g). Part F asks what would happen if more water was added. My...
- Thu Jan 28, 2021 8:33 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook Question 5.35
- Replies: 1
- Views: 148
Textbook Question 5.35
Hey guys! I have a few questions on textbook question #5.35. First of all, I don't understand how exactly to write the balanced equation for part a. I understand that the base equation is A(g) → B(g) + C(g) because the graph is showing the decomposition of A into B and C. What I don't really underst...
- Sat Jan 23, 2021 9:11 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Rounding E Values in ICE charts
- Replies: 17
- Views: 707
Re: Rounding E Values in ICE charts
Hey Victoria! Basically, we are allowed to round the equilibrium value in an ICE chart when Kc < 1.0x10^-3. One way to double check if rounding the equilibrium value in the ICE chart was appropriate is to make sure that the X value you calculated using the rounding is less than 5% of the initial con...
- Sat Jan 23, 2021 9:03 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Ka correlation to strength of an acid
- Replies: 30
- Views: 2323
Re: Ka correlation to strength of an acid
Hey Aliya! Basically, the Ka value is a measurement of how much an acid dissociates in solution. Therefore, the higher the Ka value, the more the acid has dissociated, the higher the concentration of hydronium ions in solution, and the stronger the acid. Similarly, the lower the Ka value the weaker ...
- Sat Jan 23, 2021 8:56 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: pKa and Ka
- Replies: 27
- Views: 1017
Re: pKa and Ka
Hey Lilly! Essentially, whenever anything has a "p" in front of it, it is telling you to take the negative log of the given value. So yes, pKa is just the negative log of Ka. However, the two are related in the sense that a smaller pKa value means the Ka value is relatively large and vice ...
- Sat Jan 23, 2021 8:52 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Solids in Ice Tables
- Replies: 11
- Views: 1043
Re: Solids in Ice Tables
Hey Cecilia!
I don't think you have to include the concentration of a solid in an ICE table because it's not included in the equilibrium constant. Hope this helps!
I don't think you have to include the concentration of a solid in an ICE table because it's not included in the equilibrium constant. Hope this helps!
- Thu Jan 21, 2021 10:55 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Textbook Question 5G.9 Part C
- Replies: 2
- Views: 243
Textbook Question 5G.9 Part C
Hey guys! I'm a little bit confused on the textbook question 5G.9, specifically part C. The question reads " A sample of ozone, O3, amounting to 0.10 mol, is placed in a sealed container of volume 1.0 L and the reaction 2O3(g) → 3O2 (g) is allowed to reach equilibrium. Then 0.50 mol O3 is place...
- Sat Jan 16, 2021 1:07 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Lecture #6 Question - Hydronium Concentration
- Replies: 2
- Views: 213
Lecture #6 Question - Hydronium Concentration
Hey guys! I'm a little confused about a note Dr. Lavelle added in Lecture #6. Basically he said that, when calculating the pH of a weak acid or base, if the concentration of hydronium ions is less than 1x10^-7, we are to consider the solution neutral because autoprototlysis generates 1x10^-7M H3O+. ...
- Sat Jan 16, 2021 12:59 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Conjugate Seesaw Application
- Replies: 2
- Views: 146
Conjugate Seesaw Application
Hey guys! I just wanted to make sure I am understanding how exactly to apply the conjugate seesaw. In lecture #5, Dr. Lavelle said that when you "add up" two chemical reactions, you get 2H2O(l) → H3O+(aq) + OH-(aq). I just wanted to clarify that the two chemical reactions you "add tog...
- Fri Jan 15, 2021 11:54 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Week 2 Sapling Homework - Question #5
- Replies: 4
- Views: 406
Week 2 Sapling Homework - Question #5
Hey guys! I'm having a little bit of trouble on question #5 in the Week 2 Sapling homework. The question reads "The Kb for an amine is 5.320x10^-5. What percentage of the amine is protonated if the pH of a solution of the amine is 9.701?". -For starters, I wrote out a formula for the chemi...
- Fri Jan 15, 2021 10:50 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Week 2 Sapling Homework - Question #1
- Replies: 3
- Views: 242
Week 2 Sapling Homework - Question #1
Hey guys! I'm a little confused on how to solve question #1 on the Week 2 Sapling homework. My question states "If the Ka of a monoprotic weak acid is 9.0X10^-6, what is the pH of a 0.14M solution of this acid?". I'm not really sure how to relate Ka to pH with the given information. If som...
- Fri Jan 15, 2021 10:43 pm
- Forum: Polyprotic Acids & Bases
- Topic: What Does Monoprotic Mean?
- Replies: 16
- Views: 1075
What Does Monoprotic Mean?
Hey guys!
A couple of the questions in the Week 2 Sapling homework say that a given substance is a monoprotic weak acid. I was wondering, what does monoprotic mean in terms of the acid? Thanks in advance!
A couple of the questions in the Week 2 Sapling homework say that a given substance is a monoprotic weak acid. I was wondering, what does monoprotic mean in terms of the acid? Thanks in advance!
- Sun Jan 10, 2021 9:18 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Q>K
- Replies: 10
- Views: 371
Re: Q>K
Hey Aishwarya! You are correct in saying that once a reaction reaches equilibrium the concentrations of products and reactants would stay the same. Essentially, when Q>K, some outside occurrence has occurred that has shifted the reaction out of equilibrium. For example, a change in temperature, the ...
- Sun Jan 10, 2021 9:08 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Q and K
- Replies: 13
- Views: 515
Re: Q and K
Hey Melissa, That is correct! We use Q when calculating the reaction quotient of a reaction that isn't at equilibrium. Because Q is calculated the same way as K ([P]/[R]), then if the reaction is at equilibrium the ratio of the concentrations of products to reactants would just be equal to K. If the...
- Sun Jan 10, 2021 9:03 am
- Forum: Ideal Gases
- Topic: P over R in the Ideal Gas Law
- Replies: 4
- Views: 205
Re: P over R in the Ideal Gas Law
Hey Bronson, I don't believe that P/R is directly proportional to K (the equilibrium constant) using the ideal gas law. The ideal gas law states PV=nRT, which can be arranged to state n/V=P/RT. This can also be written as concentration=P/RT. While both this rearranged ideal gas law and K deal with c...
- Fri Jan 08, 2021 8:41 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Increasing Pressure by Adding an Inert Gas
- Replies: 6
- Views: 887
Increasing Pressure by Adding an Inert Gas
Hey guys! I just wanted some clarification of why exactly increasing pressure by adding an inert gas doesn't move the reaction from equilibrium. I understand that the reaction doesn't move from equilibrium because the concentrations of the reactants and products don't change. Where I get confused is...
- Fri Jan 08, 2021 8:26 pm
- Forum: Ideal Gases
- Topic: Ideal Gas Definition
- Replies: 10
- Views: 655
Ideal Gas Definition
Hey guys! In Lecture #2, Dr. Lavelle mentions we are going use the ideal gas law for all gases when dealing with equilibrium calculations. I'm a little confused as to what exactly an ideal gas is? If someone could explain what an ideal gas is and how it is different than a non-ideal gas that would b...
- Sat Dec 12, 2020 1:29 pm
- Forum: Lewis Acids & Bases
- Topic: Textbook Question 6.5
- Replies: 2
- Views: 117
Textbook Question 6.5
Hey guys! I'm a little confused on textbook question 6.5, specifically part C. If someone could explain why H2O2 is the Lewis base and SO3 is the Lewis acid, that would be appreciated!
- Sat Dec 12, 2020 1:25 pm
- Forum: Calculating the pH of Salt Solutions
- Topic: Textbook Question 6D.11
- Replies: 2
- Views: 230
Textbook Question 6D.11
Hey guys! I'm unsure about how to write the chemical formulas for the aqueous solutions in textbook question 6D.11. Specifically, I don't understand how to write the equations for part E and F. If someone could explain where the answer key got the additional water molecules attached to the metal cat...
- Sat Dec 12, 2020 1:15 pm
- Forum: Amphoteric Compounds
- Topic: Textbook Question 6A.17
- Replies: 2
- Views: 182
Textbook Question 6A.17
Hey guys! I'm kinda confused on how to determine wether or not a compound is acidic, basic, or amphoteric. If someone could explain to me why, in question 6A.17, BaO is basic, SO3 is acidic, and As2O3 and Bi2O3 are ampotheric that would be great. Also, if there are any guidelines for determining if ...
- Sat Dec 12, 2020 1:06 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Final Content-Naming Acids
- Replies: 2
- Views: 169
Final Content-Naming Acids
In a lot of the textbook problems that go along with the acid and base section, we were supposed to either know the formula of an acid from its name or name an acid from its formula. I don't remember going over this in class. I'm not sure if I either missed it in lecture or if we actually didn't go ...
- Fri Dec 11, 2020 10:40 pm
- Forum: Conjugate Acids & Bases
- Topic: Textbook Question 6A.3
- Replies: 1
- Views: 217
Textbook Question 6A.3
Hey guys! The textbook problem question 6A.3 deals with writing chemical equations and identifying the conjugate acid-base pairs. I just wanted to make sure that I am understand parts b and d correctly. For part b, you have to write the chemical equation for anilinium ion (C6H5NH3+), in water. I jus...
- Thu Dec 10, 2020 11:41 pm
- Forum: Hybridization
- Topic: Textbook Question 2.45
- Replies: 1
- Views: 118
Textbook Question 2.45
Hey guys! I'm a little confused on question 2.45 from the textbook. I understand how to draw the Lewis structure and identify the sigma and pi bonds. Where I get confused is the hybridization of each lone pair. Specifically, what I don't understand is where the number before the hybridization comes ...
- Sun Dec 06, 2020 10:25 pm
- Forum: Industrial Examples
- Topic: Coordination compounds as Chemotherapy drugs
- Replies: 9
- Views: 1841
Re: Coordination compounds as Chemotherapy drugs
Hey Arubal! In Lecture #24 Dr. Lavelle talks about a chemotherapy drug called cisplatin. I would assume this is what the syllabus is referring too, especially since the textbook doesn't talk about any additional chemotherapy drugs. Basically, we learned that the coordination compound cisdiamine-dich...
- Sun Dec 06, 2020 10:05 pm
- Forum: Naming
- Topic: Steps for Naming Coordination Compounds
- Replies: 9
- Views: 1671
Re: Steps for Naming Coordination Compounds
Hey Jolie! Basically the general "formula" if you will for naming coordination compounds is Greek prefix-ligand name + transition metal cation name (roman numeral) + anion name + Greek prefix-hydrate. This is slightly confusing just looking at it, but once you get the hang of naming it get...
- Sun Dec 06, 2020 5:10 pm
- Forum: Bronsted Acids & Bases
- Topic: Why the Bronsted Definition Is Less Fundamental Than the Lewis Definition
- Replies: 2
- Views: 159
Why the Bronsted Definition Is Less Fundamental Than the Lewis Definition
Hey guys! In Lecture #26, Dr. Lavelle said that the Bronsted definition of acid and bases isn't as fundamental as the Lewis definition because not every reaction involves protons. I'm a little confused on how a chemical reaction involving an acid or a base can take place without the involvement of p...
- Sun Dec 06, 2020 5:04 pm
- Forum: Bronsted Acids & Bases
- Topic: Proton Donor/Acceptor
- Replies: 2
- Views: 152
Proton Donor/Acceptor
Hey guys! I was hoping that one of you can clarify why exactly something is a proton donor or a proton acceptor. I was thinking that a molecule is a proton donor and therefor a Bronsted acid when one of its hydrogens forms a hydroxide ion because the protons in said hydrogen and being transferred (o...
- Sun Dec 06, 2020 4:54 pm
- Forum: Naming
- Topic: Anion Naming
- Replies: 7
- Views: 414
Anion Naming
Hey guys! I just wanted to clarify something about naming anions that interact with coordination compounds. On Sapling, I had to name [Co(NH3)5Cl]Cl2. I understand how to name the coordination compound inside the brackets, but I was a little confused about how to name the anion outside the brackets....
- Sun Nov 29, 2020 12:38 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: sigma vs pi bonds
- Replies: 33
- Views: 2160
Re: sigma vs pi bonds
Hey Queena! A sigma bond occurs when two orbitals interact end-to-end and form a bond. A pi bond occurs when two orbitals overlap side-by-side and form a bond. Pi bonds can only form if an atom's electron configuration includes a d-orbital because without a d-orbital there is only one orbital, the s...
- Sun Nov 29, 2020 12:15 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: sapling #12
- Replies: 13
- Views: 833
Re: sapling #12
Hey Jade! I think where you are going wrong is the number of bonds on carbon. Remember carbon's electron configuration does not have a d-orbital so a carbon atom cannot have more than four bonds. Taking this into consideration, all you have to do is move one of the hydrogens that is bound to the car...
- Sun Nov 29, 2020 12:04 am
- Forum: Hybridization
- Topic: Confused on hybridization conceptually
- Replies: 9
- Views: 645
Re: Confused on hybridization conceptually
Hey Jessica! Essentially hybridization is very similar to what the name suggests. In hybridization, the orbitals of an atom are hybridizing or, in other words, mixing together. Basically, when bonding, atoms may not have enough unpaired electrons in their valence orbitals to create the bonds they ne...
- Sat Nov 28, 2020 11:48 pm
- Forum: Hybridization
- Topic: dsp^3 vs sp^3d
- Replies: 2
- Views: 110
dsp^3 vs sp^3d
Hey guys! I was just wondering why some people write the hybridization of an atom like dsp^3 and not sp^3d? I was thinking that maybe people write the hybridization like dsp^3 with the 'd' out front because, in electron configurations, the d-orbitals fill up after the s-orbitals. If someone could le...
- Sat Nov 28, 2020 11:40 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Clarification on Shape vs Arrangement
- Replies: 5
- Views: 260
Re: Clarification on Shape vs Arrangement
Hey Emily! You are correct in saying that lone pairs do influence molecular shape. The amount of lone pairs and amount of bonding pairs both contribute to the molecular shape of a molecule (even though naming has to do with the amount of bonding pairs). What the textbook means by stating "Elect...
- Sun Nov 22, 2020 2:28 pm
- Forum: Ionic & Covalent Bonds
- Topic: Covalent Character
- Replies: 33
- Views: 1632
Re: Covalent Character
I'm pretty sure that when determining which ionic molecules display the most covalent character, you just look at the difference in electronegativity. The smaller the difference in electronegativity, the more covalent character the molecule has and vise versa. One way to determine this without the e...
- Sun Nov 22, 2020 2:22 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Best Formal Charge Equations
- Replies: 24
- Views: 1150
Re: Best Formal Charge Equations
Hey Jaclyn! The formula for formal charge that Dr. Lavelle gives in lectures is: formal charge = valence electrons - ((shared electrons/2) + lone pair electrons). While this formula works, it is a little hard to remember. Instead of this formula, I like to think of formal charge as: formal charge = ...
- Tue Nov 17, 2020 9:13 pm
- Forum: Octet Exceptions
- Topic: Expanded Octet
- Replies: 2
- Views: 125
Expanded Octet
Hey guys! I have a question regarding expanded octets. I understand that atoms of elements in period three or below have d-orbitals in their valence shells that can accommodate more than 8 electrons. What I don't understand is exactly how many more electrons these elements can accommodate/how many m...
- Mon Nov 16, 2020 10:20 pm
- Forum: Dipole Moments
- Topic: Induced Dipole-Induced Dipole Interaction and Boiling Point
- Replies: 2
- Views: 119
Induced Dipole-Induced Dipole Interaction and Boiling Point
Hey guys! I don't understand how exactly the strength of an induced dipole-induced dipole interaction and boiling point relate to each other. If you could explain how these two correlate and how you would go about figuring out the boiling point of a substance (or rather figuring out if it has a high...
- Mon Nov 16, 2020 10:17 pm
- Forum: Trends in The Periodic Table
- Topic: Polarizing Power
- Replies: 1
- Views: 168
Polarizing Power
Hey guys! I'm quite confused about the trends for polarizing power on the periodic table. I understand that polarizing power decreases as you go down a period on the periodic table because the radius of the atom increases and therefor the nucleus' pull on the electrons is not as strong. Where I get ...
- Fri Nov 13, 2020 11:38 pm
- Forum: Dipole Moments
- Topic: Hydrogen Bonds
- Replies: 6
- Views: 328
Re: Hydrogen Bonds
Hydrogen bonds aren't a concrete bond, but rather a favorable electrostatic attraction. This attraction has an energy of approximately -20 kJ/mol.
- Fri Nov 13, 2020 11:33 pm
- Forum: Dipole Moments
- Topic: Strength of Induced Dipole-Induced Dipole Interaction
- Replies: 1
- Views: 52
Strength of Induced Dipole-Induced Dipole Interaction
Hey guys! In Lecture #18, Dr. Lavelle talks about how the shape of molecules contributes to the total strength of the interaction. While I understand how the shape of molecules correlates to the strength of the interaction, I'm confused on what the strength of the interaction actually means. It is r...
- Fri Nov 13, 2020 11:23 pm
- Forum: Dipole Moments
- Topic: Strength of Dispersion Forces
- Replies: 2
- Views: 158
Strength of Dispersion Forces
Hey guys! I'm a bit confused on how exactly the strength of dispersion forces relates to the number of electrons and the state of the substance. In Lecture #18, Dr. Lavelle says that the strength of dispersion forces explains why elements are at different states at room temperature. He says that thi...
- Fri Nov 13, 2020 11:12 pm
- Forum: Polarisability of Anions, The Polarizing Power of Cations
- Topic: Electron Distortion and Polarizing Power Periodic Trend
- Replies: 2
- Views: 135
Electron Distortion and Polarizing Power Periodic Trend
Hey guys! I just want to make sure I'm understanding electron distortion and polarizing power correctly. Basically, in an ionic bond the cation exerts electrostatic attraction on the electrons surrounding the anion, pulling the electrons towards itself and therefor distorting them? And when looking ...
- Fri Nov 13, 2020 10:43 pm
- Forum: Resonance Structures
- Topic: Delocalized Electrons
- Replies: 7
- Views: 372
Delocalized Electrons
In Lecture #14, Dr. Lavelle introduced the idea that the electrons involved in resonance are delocalized. My question is, what does it mean when an electron is delocalized? Thanks in advance!
- Sun Nov 08, 2020 1:09 pm
- Forum: Resonance Structures
- Topic: Question about Resonance Def
- Replies: 5
- Views: 371
Re: Question about Resonance Def
Hey Noelle! Resonance is the idea that Lewis structures can have multiple bonds (ie not single bonds) in different locations. Basically, if you're looking at a Lewis structure and it has a multiple bond that can be placed somewhere else without creating a different molecule, there is resonance. This...
- Sun Nov 08, 2020 12:58 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Lecture O Formal Charge Ex
- Replies: 4
- Views: 337
Re: Lecture O Formal Charge Ex
Hey Alison! The first thing to know when calculating formal charge is the formal charge equation. The equation is as follows: formal charge = V (number of valence electrons for the bound atom) - ( (shared electrons/2) + L (number of lone pair electrons)) In this lecture, Dr. Lavelle calculated the f...
- Sun Nov 08, 2020 12:37 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: Formal Charge Equation
- Replies: 16
- Views: 641
Re: Formal Charge Equation
In the formal charge equation, L represents the number of lone pair electrons on the given bound atom. To find L given a Lewis structure, you just count the number of dots next to the atom. The number of dots is equal to the value L. Hope this helps!
- Sat Nov 07, 2020 4:17 pm
- Forum: Resonance Structures
- Topic: Separate and Identifiable Bonds
- Replies: 2
- Views: 124
Separate and Identifiable Bonds
Hey guys! I just had a quick question from Lecture #14. When talking about delocalized electrons, Dr. Lavelle says that benzene is more stable than a molecule with three separate and identifiable single bonds and three separate and identifiable double bonds. In regards to the molecule benzene is bei...
- Sat Nov 07, 2020 4:13 pm
- Forum: Octet Exceptions
- Topic: Octet Exception for H, He, Li, and Be
- Replies: 5
- Views: 184
Octet Exception for H, He, Li, and Be
Hey guys! I just want to make sure that I truly understand the octet exception for the first four elements. When looking at the electron configurations for these elements, the valence electron is in the s subshell (1s for H and He and 2s for Li and Be), and this is why these elements defy the octet ...
- Sun Nov 01, 2020 2:25 pm
- Forum: Trends in The Periodic Table
- Topic: Oxygen and Ionization Energy
- Replies: 9
- Views: 559
Re: Oxygen and Ionization Energy
Hey Jenny! The answer to your question can be found by looking at the electron configuration of oxygen, nitrogen, and fluorine. Nitrogen has 3 electrons in the 2p subshell, oxygen has 4 electrons in the 2p subshell, and fluorine has 5 electrons in the 2p subshell. According to Hund's Rule, nitrogen ...
- Sun Nov 01, 2020 2:10 pm
- Forum: Trends in The Periodic Table
- Topic: Sapling HW #30
- Replies: 6
- Views: 328
Re: Sapling HW #30
Hey Sahiti! To answer this question, you have to remember two things. First of all, the ionic radius of a cation is going to be smaller than the radius of the parent atom because the electrostatic attraction is going to be higher per electron, thus pulling the electrons in tighter to the nucleus. Th...
- Sat Oct 31, 2020 12:55 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: 3d and 4s Orbital
- Replies: 3
- Views: 195
3d and 4s Orbital
In Lecture #11, Dr. Lavelle talks about how electrons will enter the 4s orbital before the 3d orbital because it requires less energy. I understand this, but what I don't understand is how, for multi-electron atoms with an atomic number larger than 20, the 4s orbital is higher in energy than 3d. How...
- Fri Oct 30, 2020 8:59 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Calculating M(L)
- Replies: 2
- Views: 88
Calculating M(L)
Hey guys! I'm a little confused about how exactly you calculate the possible values for M(L) given L. Just to make sure I'm understanding it correctly, the possible values for M(L) are the range of whole numbers between positive L and negative L? For example, if L=3, the possible values for M(L) are...
- Tue Oct 27, 2020 9:22 pm
- Forum: Properties of Electrons
- Topic: The Wave Model and Quantized Energy States
- Replies: 2
- Views: 148
The Wave Model and Quantized Energy States
In my notes from Lecture #8, I wrote "The wave model explains why electrons have quantized energy states in atoms as observed by experimental observation". Upon reviewing, I am confused as to how exactly the wave model relates to the quantized energy states of electrons. If someone could e...
- Sat Oct 24, 2020 1:10 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: 1B.21 Clarification
- Replies: 3
- Views: 159
Re: 1B.21 Clarification
Hey Natalie! I'm a little confused with what you mean here, so I'll tell you what I did for question 1B.21 and maybe it will match up to your though process. First, I converted the given mass (5.15 oz) from ounces to grams. I also converted the given velocity (92 mi/h) from miles per hour to meters ...
- Sat Oct 24, 2020 1:02 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Problem 1 B.27
- Replies: 2
- Views: 91
Re: Problem 1 B.27
Hey Melody! The first step to this problem is calculating the uncertainty of the bowling ball's momentum using the formula: Δp = (mass(m)) x Δv. The uncertainly of the velocity is going to be 5.0 m/s because as the problem states, the velocity is 5.00 ± 5.0 m/s. This shows that the uncertainly in ve...
- Sat Oct 24, 2020 12:54 pm
- Forum: Heisenberg Indeterminacy (Uncertainty) Equation
- Topic: Problem 1B. 25
- Replies: 1
- Views: 74
Re: Problem 1B. 25
Hey Marcus! The first thing you must do for this problem is convert the diameter of the atom from pm to m. Then, you plug in values to the Heisenberg indeterminacy equation that states (Δp)(Δx) ≥ (h/(4π)). You are solving for Δp. Δx is equal to the diameter of the atom in meters, and h is Plank's co...
- Sat Oct 24, 2020 12:45 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Lecture 10/16
- Replies: 4
- Views: 208
Re: Lecture 10/16
The sign for the energy switched from negative to positive because the first calculations gave us the energy lost by the electron as it transitioned between the levels. The sign for this energy is negative because the energy was lost. The sign for the energy then switched to positive because we were...
- Sat Oct 24, 2020 12:39 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Textbook Question 1B.15
- Replies: 3
- Views: 127
Re: Textbook Question 1B.15
Hey Evonne! To solve part A, you first find the electron's momentum using the formula: momentum(p) = (mass(m)) x (velocity(v)). Make sure to convert the given velocity from kg/s to m/s. Then, you use the momentum to find the energy of the electron with the formula: energy(E) = (momentum(p)) x (speed...
- Sun Oct 18, 2020 1:16 am
- Forum: Photoelectric Effect
- Topic: Work Function
- Replies: 6
- Views: 236
Re: Work Function
Yes, the work function (which is also referred to as the threshold energy) is the amount of energy needed to remove an electron from a given metal during a photoelectric experiment.
- Sun Oct 18, 2020 1:13 am
- Forum: Photoelectric Effect
- Topic: Excess energy
- Replies: 20
- Views: 619
Re: Excess energy
This equation is used to calculate the kinetic energy of an electron, also known as the excess energy, in a photoelectric experiment.
- Sun Oct 18, 2020 1:08 am
- Forum: Photoelectric Effect
- Topic: Textbook Problem 1A9
- Replies: 4
- Views: 322
Re: Textbook Problem 1A9
Hey Isabel! There are actually only two formulas you need to complete this problem so it's not too complicated once you get them. -The first formula is the formula for wavelength. The formula is wavelength = (c (speed of light)) / (v (frequency)). Just a note, the speed of light is equal to 3.00 x 1...
- Sun Oct 18, 2020 12:54 am
- Forum: Photoelectric Effect
- Topic: When are electrons excited vs ejected
- Replies: 16
- Views: 1485
Re: When are electrons excited vs ejected
Electrons are excited during atomic spectroscopy when they go from one energy level to another. They are ejected during the photoelectric experiment when the goal is to measure how much energy is required to remove electrons from different metals.
- Sun Oct 18, 2020 12:50 am
- Forum: Photoelectric Effect
- Topic: Light Intensity
- Replies: 23
- Views: 570
Light Intensity
Just to clarify, when talking about increasing the light intensity during the photoelectric experiment, the scientists were just increasing the brightness of the light? They weren't changing the frequency/wavelength of the light?
- Fri Oct 09, 2020 5:53 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Textbook question E.1
- Replies: 7
- Views: 268
Re: Textbook question E.1
Hey! The first step to completing this problem is finding the number of silver atoms in 1.00 mol Ag because you need to know how many atoms you are connecting. This is a simple conversion using Avogadro's number (the number of atoms/molecules in one mole of a substance). All you do is multiply 1.00 ...
- Fri Oct 09, 2020 5:35 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: sapling hw #7
- Replies: 17
- Views: 701
Re: sapling hw #7
Hey! This problem is actually easier than you might think. I know I was overthinking it before I realized that it's just multiplication and subtraction. The first thing you have to do is figure out the mass of calcium chloride. It is given than the mixture contains 32.5% calcium chloride, so all you...
- Fri Oct 09, 2020 5:22 pm
- Forum: Empirical & Molecular Formulas
- Topic: Fundamentals G25
- Replies: 3
- Views: 136
Re: Fundamentals G25
Hey! This problem took me a while to figure out too, so you're not alone haha. Anyways, the first thing I did was figure out the molarity of the diluted solution. I did this by multiplying the original molarity, 0.10 M, by (1/2)^90 because you are diluting the original molarity by half each time you...