Search found 38 matches
- Sun Mar 19, 2023 1:44 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: when to approximate
- Replies: 11
- Views: 499
Re: when to approximate
If k is less than 10^-3 it is ok to approximate. This is to say that the change of x would be so small it is irrelevant but not that there is no change. You would not put zero in for x but rather ignore the change of x in your (presumably) denominator. You can check if your approximation was okay by...
- Sun Mar 19, 2023 1:42 am
- Forum: Ideal Gases
- Topic: Gas constant R
- Replies: 14
- Views: 1843
Re: Gas constant R
Do the math paying close attention to the units being used. Everything needs to carefully cancel out in order for your answer to be valid. if one of the gas constants has a unit not given to you and not being asked for, it is the wrong one!
- Sun Mar 19, 2023 1:41 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Le chatelier's principle regarding pressure
- Replies: 10
- Views: 1212
Re: Le chatelier's principle regarding pressure
Adding gas to a system to change the pressure does not change partial pressures and therefore has no affect. Decreasing the volume however by shrinking the container (compression) would shift the equilibrium to the side with less moles.
- Sun Mar 19, 2023 1:38 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: work done on a system
- Replies: 6
- Views: 692
Re: work done on a system
This very much depends on the information given in the question. Sometimes the question might directly give you this value. Oftentimes you will need to simply find the moles by dividing the mass by the grams of one mole of something. Other times it might give you other information that would require...
- Sun Mar 19, 2023 1:34 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: week3- Enthalpy of formation vs standard enthalpy
- Replies: 5
- Views: 547
Re: week3- Enthalpy of formation vs standard enthalpy
Which one you use relies on the information given. Delta H is just your normal change in enthalpy and is very often the subject of a question. It takes very little into account. Delta H standard is the change in enthalpy only under standard conditions (pressure and temp). The delta h of formation is...
- Sun Mar 19, 2023 1:31 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Is deltaH > deltaU at equilibtrium?
- Replies: 3
- Views: 474
Re: Is deltaH > deltaU at equilibtrium?
Under constant pressure delta H and q are equal to one another. U=q+w and therefore it can depend on whether w or q are equal to one another. At equilibrium neither qualities would necessarily be equal to zero. I think the question gave a little more information. It might have been that it stated on...
- Sun Mar 19, 2023 1:28 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Entropy vs. Enthalpy
- Replies: 12
- Views: 1219
Re: Entropy vs. Enthalpy
The question should be relatively clear on which of the two it is asking about. Both will be about the change in their values but enthalpy is the heat or energy of a system and entropy is the disorder or amount of positions something can be in. Most questions will use the two terms or will show delt...
- Sun Mar 19, 2023 1:25 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Isolated Systems
- Replies: 5
- Views: 507
Re: Isolated Systems
Work will always be zero in an isolated system because an isolated system cannot be changed. No exchange of mass or energy can be done with an isolated system so no work can be done on one or by one.
- Sun Mar 19, 2023 1:23 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpies
- Replies: 8
- Views: 572
Re: Bond Enthalpies
Bond enthalpies by definition are the energy required to break a specific bond. A negative enthalpy would be the release of energy and is not the same thing. However, the amount of energy required to break a bond is the same amount of energy required to create that bond and you can therefore just fl...
- Sun Mar 19, 2023 1:21 am
- Forum: Phase Changes & Related Calculations
- Topic: Phase Changes
- Replies: 6
- Views: 665
Re: Phase Changes
I'm not entirely sure what you mean by the greatest. If you mean how much energy they require, then of course sublimation requires much more energy than vaporization because it would include the necessary energy for both fusion and vaporization. It is two phase changes at once effectively. There is ...
- Sun Mar 19, 2023 1:07 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Salt Bridge Role
- Replies: 8
- Views: 671
Re: Salt Bridge Role
The salt bridge attempts to maintain a neutrality of charges and prevents a build up of negative or positive charges in one side of lets say a galvanic cell. With electrons constantly being sent from one side to another, there would obviously be too many negative charges on the receiving end and too...
- Sun Mar 19, 2023 12:52 am
- Forum: Balancing Redox Reactions
- Topic: Balancing in Acidic vs Basic
- Replies: 6
- Views: 2076
Re: Balancing in Acidic vs Basic
The steps remain largely the same. You have to add water to the equation regardless but to balance out the extra hydrogens you add H+ ions to acidic solutions and OH- ions to basic solutions. Other than that everything else doesn't change based on it being acidic or basic.
- Sun Mar 19, 2023 12:32 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Ea Dependence
- Replies: 4
- Views: 532
Re: Ea Dependence
That is correct. The higher the activation energy the more susceptible a reaction is to temperature changes. Higher temperatures will affect something with a higher activation energy more than something with a lower activation energy.
- Sun Mar 19, 2023 12:05 am
- Forum: Zero Order Reactions
- Topic: Graphs
- Replies: 4
- Views: 513
Re: Graphs
The graphs would each be shown with a straight line as graphing one part of any order against time would always result in linearity.
- Sun Mar 19, 2023 12:03 am
- Forum: *Enzyme Kinetics
- Topic: Rate law
- Replies: 8
- Views: 617
Re: Rate law
Enzymes are not directly part of the rate as they are not used up. They are similar to intermediates in that they are outside necessary factors to a reaction occurring.
- Sun Mar 19, 2023 12:01 am
- Forum: Second Order Reactions
- Topic: Orders in Equations
- Replies: 5
- Views: 526
Re: Orders in Equations
Memorizing them is in your best interests but as a general rule of thumb I would say that zero order reactions are normally the simplest and most straight forward. First order reactions are more difficult to guess and should probably be memorized but second order reactions typically square something...
- Sat Mar 18, 2023 11:51 pm
- Forum: Biological Examples
- Topic: Enzymes and biological kinetics
- Replies: 4
- Views: 908
Re: Enzymes and biological kinetics
Enzymes are proteins that catalyze a reaction to make them occur faster. They can also regulate when and how reactions occur. They lower the activation energy of reactions so they can occur more frequently and quicker. Occasionally reactions would be impossible without enzymes but often they make re...
- Sat Mar 18, 2023 11:44 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Achieve Week 8-10 #20
- Replies: 11
- Views: 1272
Re: Achieve Week 8-10 #20
You did the rest of this question all correct you just missed the conversion from kj to joules to match the rate constant. Your answer will end up a very large number. Just make sure to do the same thing for both temperatures.
- Sat Mar 18, 2023 11:40 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Achieve Week 8-10: Chemical Kinetics #13
- Replies: 7
- Views: 625
Re: Achieve Week 8-10: Chemical Kinetics #13
The rate of formation is determined by the slow step giving rate=l[I-][HClO] The forward and reverse rates can be set equal to one another because the reaction is at equilibrium. k[ClO-]=k[HClO][OH-]. Then we can solve for HClO and substitute that answer into our original rate equation. We then end ...
- Sat Mar 18, 2023 11:21 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: Spontaneous Reaction
- Replies: 6
- Views: 840
Re: Spontaneous Reaction
You would need the delta G value to be able to determine if a reaction is spontaneous. Just having the delta h value isn't enough because its spontaneity would depend on delta S as well, or the entropy value. The delta U would also not be able to tell you if a reaction is spontaneous or not.
- Sat Mar 18, 2023 11:12 pm
- Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
- Topic: What is Entropy?
- Replies: 11
- Views: 1784
Re: What is Entropy?
Hello, entropy is the degree of disorder of something. When we look at it in this class it normally refers to a reaction and the change in entropy. To better understand this, when a gas is highly pressurized the particles are moving faster and there is more disorder, hence higher entropy. It can als...
- Fri Mar 17, 2023 5:40 pm
- Forum: General Rate Laws
- Topic: Achieve Weeks 8-10, #1
- Replies: 4
- Views: 151
Re: Achieve Weeks 8-10, #1
reactants are negative because their concentration will be decreasing whereas products will be positive because theirs is increasing
- Fri Mar 17, 2023 5:10 pm
- Forum: General Rate Laws
- Topic: Achieve Week 10 #4
- Replies: 8
- Views: 319
Re: Achieve Week 10 #4
To understand the orders you must think of the number of species interacting at once. The rate equation for zero order is rate=k. We are trying ot find our answer in concentration over time. A common unit for that is molarity/seconds which is what we will try and solve for and put in as our rate. Fo...
- Sun Mar 05, 2023 11:46 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Reaction Enthalpy pos/neg signs
- Replies: 5
- Views: 674
Re: Reaction Enthalpy pos/neg signs
it is important to understand that the value being positive means that something is endothermic and negative meaning it is exothermic. Questions given will often give the value and therefore there is nothing to figure out. other times it will refer to bond enthalpy values and ask you to find the tot...
- Sun Mar 05, 2023 11:43 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpy
- Replies: 9
- Views: 694
Re: Bond Enthalpy
Bond enthalpy is the energy required to break a bond and is therefore always positive when seen in charts. However, this value tells you both the energy required to break and create a bond as they are simply the inverse of one another. Negative bond enthalpy value is what is required to create the s...
- Sun Mar 05, 2023 11:40 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Forming and breaking bonds
- Replies: 12
- Views: 767
Re: Forming and breaking bonds
It always requires an input of heat and energy to break a bond. This would therefore not be spontaneous and must be endergonic and exothermic. Creating a bond releases heat and is therefore spontaneous making it exothermic.
- Sun Feb 26, 2023 11:39 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: delta U
- Replies: 18
- Views: 935
Re: delta U
Delta U is the change in the internal energy of a system. This can be added and does not depend on any path, therefore it is a state function.
- Sun Feb 26, 2023 11:38 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Entropy
- Replies: 7
- Views: 364
Re: Entropy
The sheet of constants includes that!
- Sun Feb 26, 2023 11:37 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond enthalpy value
- Replies: 4
- Views: 192
Re: Bond enthalpy value
Bond enthalpy values are always positive because it always requires an input of energy to break a bond, which is effectively what a bond enthalpy value is. It is technically the amount of energy stored in the bond and it requires as much to break it.
- Sun Feb 19, 2023 9:05 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: spontaneity
- Replies: 7
- Views: 197
Re: spontaneity
Spontaneity refers to if a reaction can occur on it's own, without an input of energy. This could be called a reaction occurring spontaneously. Reactions that can occur spontaneously have a negative delta G value and release energy. Reactions that do not occur spontaneously require an input of energ...
- Sun Feb 19, 2023 9:02 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Nonlinear and Linear Molecules
- Replies: 4
- Views: 202
Re: Nonlinear and Linear Molecules
Hello. Utilizing the VSEPR rules such as those in this image will help you.
- Sun Feb 19, 2023 8:59 pm
- Forum: Phase Changes & Related Calculations
- Topic: phase changes
- Replies: 4
- Views: 206
Re: phase changes
Hello. Every substance is different and it also depends on what phase change is being done. Q=mL is the formula for heat released and L is a "latent heat coefficient." Every substance would undergo phase change at a set specific temperature so naturally the heat released or absorbed is dif...
- Sun Jan 29, 2023 9:21 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Midterm
- Replies: 20
- Views: 782
Re: Midterm
how many questions are on the midterm? which lectures exactly will be covered?
- Sun Jan 29, 2023 9:19 pm
- Forum: Administrative Questions and Class Announcements
- Topic: How to find my posts
- Replies: 163
- Views: 230959
Re: How to find my posts
if you click on your name you can find all your previous posts
- Sun Jan 29, 2023 9:17 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Textbook Inquiry [ENDORSED]
- Replies: 29
- Views: 82905
Re: Textbook Inquiry [ENDORSED]
yes you can download it on the website! We can access it for a few years if i recall correctly.
- Sun Jan 22, 2023 10:49 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Acids and Bases
- Replies: 264
- Views: 265094
Re: Acids and Bases
There is a section under 14A. There are various videos and links for acids and bases in 14B though.
- Sun Jan 22, 2023 10:47 pm
- Forum: Administrative Questions and Class Announcements
- Topic: New account for Chem 14B?
- Replies: 41
- Views: 62603
Re: New account for Chem 14B?
The same account works just fine!
- Sun Jan 22, 2023 10:46 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Lectures
- Replies: 2
- Views: 103
Lectures
Is there anyway we can access lecture slides?