A is the pre-exponential factor. It is the fraction of molecules that would react if the activation energy was zero (if Ea is 0, e^0/RT would be 1 so your arrhenius equation would be k=a).
A is usually determined with experimental data, since it's different for different reactions.
Search found 63 matches
- Mon Mar 19, 2018 3:15 am
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: arrhenius equation
- Replies: 1
- Views: 436
- Mon Mar 19, 2018 3:09 am
- Forum: Balancing Redox Reactions
- Topic: periodic trends
- Replies: 3
- Views: 648
Re: periodic trends
the oxidizing power increases as you go to the right and up (similar to electronegativity). The reducing power is the opposite, with elements like lithium being a strong one.
- Sun Mar 18, 2018 10:39 am
- Forum: Balancing Redox Reactions
- Topic: test 2
- Replies: 5
- Views: 834
Re: test 2
you use the deltaG=-nFE equation.
Fe2+ + e- -> Fe2+ deltaG1 = -(1)(F)(0.77)
Fe2+ + 2e- => Fe(s) deltaG2 = -(2)(F)(-0.44)
Add them up, then solve for E.
deltaG1+deltaG2 = -(3)(F)(E).
Which is -0.037 V.
Fe2+ + e- -> Fe2+ deltaG1 = -(1)(F)(0.77)
Fe2+ + 2e- => Fe(s) deltaG2 = -(2)(F)(-0.44)
Add them up, then solve for E.
deltaG1+deltaG2 = -(3)(F)(E).
Which is -0.037 V.
- Sun Mar 11, 2018 11:09 pm
- Forum: Balancing Redox Reactions
- Topic: redox
- Replies: 6
- Views: 917
Re: redox
LEO the lion says GER.
a loss of electrons is oxidation, so the oxidizing agent is what makes the loss of electrons happen, aka what gets more electrons by oxidizing something else.
The reducing agent is what causes the gain of electrons, so it gives up electrons to reduce something else.
a loss of electrons is oxidation, so the oxidizing agent is what makes the loss of electrons happen, aka what gets more electrons by oxidizing something else.
The reducing agent is what causes the gain of electrons, so it gives up electrons to reduce something else.
- Sun Mar 11, 2018 10:34 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Pre-equiliibrium?
- Replies: 3
- Views: 588
Re: Pre-equiliibrium?
pre-equilibrium: basically when the process is not at equilibrium. Since the rate of reaction measures how fast the reaction progresses UNTIL equilibrium (before it reaches equilibrium)
- Sun Mar 11, 2018 10:33 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: k and Ea
- Replies: 4
- Views: 2040
Re: k and Ea
you can think about it this way... the equilibrium constant k is basically products/reactants. If the activation energy is super high, then it's harder to form products since we have to first overcome this barrier. So when the numerator is smaller, k is smaller.
- Sun Mar 04, 2018 10:15 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: Rate determining reaction
- Replies: 3
- Views: 428
Re: Rate determining reaction
The rate determining step would be the slowest step of the reaction. You would calculate the rate based on the slower step.
- Sun Mar 04, 2018 10:12 pm
- Forum: General Rate Laws
- Topic: Rate laws
- Replies: 4
- Views: 559
Re: Rate laws
Well, we could possibly be asked to calculate the order of the reaction with respect to a certain substance given a table of concentrations.
- Sun Mar 04, 2018 10:02 pm
- Forum: First Order Reactions
- Topic: Derivations
- Replies: 6
- Views: 802
Re: Derivations
Also, as general comprehension of formulas, we should know the theory behind where they came from.
- Sun Mar 04, 2018 9:59 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3654059
Re: Post All Chemistry Jokes Here
Dang girl you are a 10.
On a pH scale.
Because you are basic.
On a pH scale.
Because you are basic.
- Thu Mar 01, 2018 12:16 am
- Forum: Kinetics vs. Thermodynamics Controlling a Reaction
- Topic: 15.3 [ENDORSED]
- Replies: 7
- Views: 874
Re: 15.3 [ENDORSED]
Since it 10^-3 mol is the same as 1 mmol, it's the same thing. Convention maybe just wanted the answer to be in standard moles.
- Thu Feb 22, 2018 1:10 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 14.107
- Replies: 1
- Views: 328
14.107
14.107 What range (in volts) does a voltmeter need to have to measure pH in the range of 1 to 14 at 25 C if the voltage is zero when pH = 7?
When using the formula E=RT/nF lnK, why is n = 1? Is it always this way, or is there something in this problem specifically that tells us we have one mol?
When using the formula E=RT/nF lnK, why is n = 1? Is it always this way, or is there something in this problem specifically that tells us we have one mol?
- Thu Feb 22, 2018 12:40 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cathode vs Anode
- Replies: 4
- Views: 638
Re: Cathode vs Anode
I think by convention you put the anode first, because then when you read it from left to right your eyes follow the flow of electrons from anode to cathode. So, oxidation (anode) -> reduction (cathode) site.
- Thu Feb 22, 2018 12:33 am
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 14.19
- Replies: 2
- Views: 401
Re: 14.19
Yeah, what's given to us is the cell potential. The question is asking for the M2/M couple, which is the cathode. So rearranging the potential = cathode-anode will give us the correct answer, -0.689+0.34=-0.349 V.
- Thu Feb 15, 2018 3:13 pm
- Forum: Phase Changes & Related Calculations
- Topic: Specific heat of water or ice?
- Replies: 6
- Views: 1125
Re: Specific heat of water or ice?
Water is only ice below 0 degrees, so we would use the specific heat of ice below that and then include the heat of fusion at 0 degrees then the specific heat of water above 0 degrees. So we use ice -> phase change -> water. Your delta temperature for the ice should have 0 as the final, and the delt...
- Thu Feb 15, 2018 3:09 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: log vs. ln [ENDORSED]
- Replies: 2
- Views: 468
Re: log vs. ln [ENDORSED]
the NERNST equation can be written with both ln and log, there's just an added constant for log. So for ln: E = E-RT/nF(lnQ) but for log: E = E-2.303RT/nF(logQ)
- Thu Feb 15, 2018 3:01 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: s vs. delta s
- Replies: 7
- Views: 1723
Re: s vs. delta s
most of the times in calculations it's delta s, because we are measuring the entropy of some reaction and therefore take the entropy of the products minus reaction (thus a change in entropy).
- Wed Feb 07, 2018 11:43 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: quiz question #7
- Replies: 1
- Views: 319
Re: quiz question #7
I don't know what "five steps of enthalpies we have to calculate" are but number 7 was about making iced-tea. So the enthalpy of fusion from ice melting is 30grams*(1mol/18.01grams)*(6010Joules/mol) which you add to the heat(q=mcDeltaT) of your now water to get the total q_ice. for referen...
- Wed Feb 07, 2018 11:33 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.1
- Replies: 4
- Views: 643
Re: 9.1
The answer is actually positive,
100/(20+273.15)=0.341 Joules/(Kelvin second)
100/(20+273.15)=0.341 Joules/(Kelvin second)
- Wed Feb 07, 2018 11:13 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.103
- Replies: 4
- Views: 582
Re: 9.103
As given, is there no way to figure out what deltaG is? In order to do this problem, is the only way to search up the deltaG of the entire reaction by some appendix?
- Wed Feb 07, 2018 10:57 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.103
- Replies: 4
- Views: 582
Re: 9.103
So how would you tell whether the equations, A and B, are spontaneous or not?
- Wed Feb 07, 2018 10:35 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.103
- Replies: 4
- Views: 582
9.103
How can we determine if a reaction is spontaneous by just looking at it? Especially in the context of this case. 9.103 A scientist proposed the following two reactions to produce ethanol, a liquid fuel: C 2H4(g) + H2O(g) -> CH3CH2OH(l) (A) C 2H6(g) + H2O(g) -> CH3CH2OH(l) + H2(g) (B) Assume standard...
- Wed Jan 31, 2018 11:51 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Midterm
- Replies: 6
- Views: 744
Re: Midterm
Both probably, but it's always helpful to understand concepts before you can carry out computations.
- Wed Jan 31, 2018 11:50 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: what exactly is free energy?
- Replies: 5
- Views: 666
Re: what exactly is free energy?
Free energy is like all the energy in the universe available to be released or consumed through reactions taking place. The Gibbs free energy is a measure of "usable" energy in the system. Basically how much energy you have available to do work. So when we have deltaG, we are looking at th...
- Wed Jan 31, 2018 11:35 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: 9.13
- Replies: 5
- Views: 655
Re: 9.13
it tells us to assume ideal gas conditions, which means we assume 1 mol of gas.
- Sun Jan 28, 2018 9:50 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Isothermal Reversible
- Replies: 3
- Views: 838
Re: Isothermal Reversible
not all isothermal reactions are reversible. for a thermodynamic process to be reversible, it must maintain equilibrium with its surroundings at all instances. So, the process must progress slowly without acceleration. The expansion of an ideal gas into a vacuum is isothermal. It is expanding into e...
- Sun Jan 28, 2018 9:23 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Cp for an ideal gas
- Replies: 2
- Views: 439
Re: Cp for an ideal gas
Here's one proof, scroll down to the second half of the page for Cp (the first half is Cv) http://physics.bu.edu/~redner/211-sp06/class24/class24_heatcap.html and also you might ask where the Energy = 3/2 * nRdeltaT comes from, which is explained conceptually in the following video: https://www.khan...
- Sun Jan 28, 2018 9:16 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Difference between systems? [ENDORSED]
- Replies: 8
- Views: 1099
Re: Difference between systems? [ENDORSED]
An open system freely exchanges energy and matter with its surroundings. The simplest example of this is boiling water, where both water can leave in the form of vapor and it gives off heat. A closed system only exchanges energy with its surroundings, so this is like boiling water with a lid on. You...
- Sun Jan 21, 2018 11:50 pm
- Forum: Student Social/Study Group
- Topic: First Test Topics
- Replies: 2
- Views: 674
Re: First Test Topics
basically, nothing about the isothermal reversible reaction calculations.
- Sun Jan 21, 2018 11:47 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Heat and systems
- Replies: 3
- Views: 554
Re: Heat and systems
Heat transfers from a higher point of temperature to a lower one. So look at a problem and determine if the system losing heat or gaining heat.
- Sun Jan 21, 2018 11:44 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Entropy of an Isolated System
- Replies: 4
- Views: 868
Re: Entropy of an Isolated System
isolated systems always go towards thermodynamic equilibrium, and that is a state with maximum entropy. An example is if you have an ice cube in a room, and the room is an isolated system, the total entropy inside the room will increase as the ice melts. The system is exchanging heat within itself a...
- Sun Jan 21, 2018 11:40 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: closed sysytem
- Replies: 3
- Views: 434
Re: closed sysytem
mercury in a thermometer: no matter can escape, but heat can. We can see that when the temperature is hot the mercury expands, causing the thermometer to have a higher reading. The mercury is affected by the heat of the surroundings. That's a simple explanation. But no matter escapes because as we s...
- Mon Jan 15, 2018 4:57 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Units of Pressure
- Replies: 3
- Views: 476
Re: Units of Pressure
Also, Dr. Lavelle noted that for our calculations we can kind of equate atm and bar since they are so similar in value.
- Mon Jan 15, 2018 4:54 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Units
- Replies: 2
- Views: 299
Re: Units
Or, you can always do dimensional analysis and see which units cancel out when calculating.
- Mon Jan 15, 2018 4:53 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy Trends
- Replies: 2
- Views: 330
Re: Enthalpy Trends
Yeah, also stable bonds like staying as such so it would take more energy to break them. A bond with a weak enthalpy would be able to dissolve without much input.
- Sat Dec 09, 2017 10:29 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Practice Test Fall 2017 [ENDORSED]
- Replies: 19
- Views: 3438
Re: Practice Test Fall 2017 [ENDORSED]
There is a question on the final practice test, number 22, that asks how many O2 molecules can myoglobin bind and how many myoglobins form a hemoglobin. I know biologically the answer is each myoglobin can bind one oxygen and hemoglobin is composed of 4 myoglobins, but what is the chemical explanati...
- Fri Dec 08, 2017 12:35 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: Acid Strength
- Replies: 5
- Views: 3051
Re: Acid Strength
I think you might be mistaken, HCl is a stronger acid than HF.
There are 7 common strong acids and HCl is on that list, HF is not.
There are 7 common strong acids and HCl is on that list, HF is not.
- Fri Dec 08, 2017 12:29 am
- Forum: Properties & Structures of Inorganic & Organic Acids
- Topic: 12.7
- Replies: 2
- Views: 531
Re: 12.7
For part a, the conjugate base to HClO3 is ClO3-. The lewis structure has a central Cl atom, connected to two oxygen atoms with double bonds and a third oxygen with a single bond. The double bonded oxygens have 2 lone pairs each while the single bond connected oxygen has 3 lone pairs (6 total lone e...
- Thu Nov 30, 2017 10:43 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Table 11.2
- Replies: 4
- Views: 543
Re: Table 11.2
K is Kp, the equilibrium constant based on the partial pressures. The relationship between Kc and Kp is Kp = Kc(RT)^delta(n). This can be derived from the ideal gas equation (PV=nRT) by letting P = nRT/V (and n/V is the concentration, so this is P = [gas]RT) and plugging that in to the Kp equation (...
- Thu Nov 30, 2017 10:09 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Units for K and Q [ENDORSED]
- Replies: 5
- Views: 2204
Re: Units for K and Q [ENDORSED]
You just have to use the same constant for all your calculations. Since the units eventually cancel out to render K unitless, it doesn't really matter as long as it's all the same (so don't use atm for one molecule and bar for another, but if you use atm for all then all the atms cancel anyways). Si...
- Wed Nov 22, 2017 1:55 pm
- Forum: Naming
- Topic: Question 17.29a
- Replies: 3
- Views: 429
Re: Question 17.29a
Ferrous means iron. Ever notice that the symbol for iron is Fe instead of like... Ir (actually iridium)? It's derived from latin. Another example is Copper, which you might expect to be Co (that's actually cobalt) but Copper is actually Cu... stands for cupric, also latin for copper. Tin is another ...
- Wed Nov 22, 2017 1:51 pm
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: 17.33 (whole)
- Replies: 3
- Views: 915
Re: 17.33 (whole)
Polydentate ligands is basically when you bind a bunch of these given molecules to a central metal atom or ion. So how many bonds does each molecule make with the metal? I'll give the easiest example, part c, which is water. This is monodentate because only the oxygen atom is a donor atom that has e...
- Thu Nov 16, 2017 9:24 pm
- Forum: Student Social/Study Group
- Topic: Post All Chemistry Jokes Here
- Replies: 9651
- Views: 3654059
Re: Post All Chemistry Jokes Here
Aren't you all glad we have this chemistry community forum? It makes 14A less of a cheMYSTERY for us all :)
- Thu Nov 16, 2017 9:16 pm
- Forum: Ionic & Covalent Bonds
- Topic: SiO2
- Replies: 4
- Views: 6109
Re: SiO2
You know that the Si-O bonds are polar because of their location on the periodic table. We know that C-O bonds are polar, since oxygen is more electronegative than carbon, and Silicon is in the same group as carbon -> Si-O bonds are also expected to be polar.
- Thu Nov 16, 2017 9:04 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: bond angle
- Replies: 4
- Views: 2273
Re: bond angle
The bond angle for something is the angle between your central atom and the two directly attached to it. For example, in water the bond angle is the angle created by H-O-H. For a trigonal bipyramidal molecule like PF5, the bond angles are either 120 or 90 degrees. See the attached graphic... It's ea...
- Thu Nov 09, 2017 1:23 pm
- Forum: Dipole Moments
- Topic: Finding Dipole Moments
- Replies: 3
- Views: 745
Re: Finding Dipole Moments
And when drawing the arrows for dipole movements, it always goes from the less electronegative atom -> more electronegative atom. It's a measure of polarity, and the large electronegativity difference, the larger dipole movement force.
- Thu Nov 09, 2017 1:17 pm
- Forum: DeBroglie Equation
- Topic: Diffraction Patterns
- Replies: 2
- Views: 365
Re: Diffraction Patterns
When waves run into each other they either contructively build or destructively become weaker. So when we measure "how much" wave we get at each location, we get a diffraction pattern that shows where waves added up and where they canceled out. The following gif representation of how diffr...
- Thu Nov 09, 2017 1:13 pm
- Forum: Dipole Moments
- Topic: Polarity
- Replies: 5
- Views: 884
Re: Polarity
You can look for either lone pair electrons or polar bonds. If we take two molecules, CO2 and H2O which may both seem to be linear in shape because they have 3 atoms each, we find that actually CO2 is linear while H2O is bent. Because the lone pair electrons on water repel the hydrogens and force a ...
- Thu Nov 02, 2017 5:35 pm
- Forum: Trends in The Periodic Table
- Topic: Diagonal relationships
- Replies: 1
- Views: 210
Re: Diagonal relationships
Many chemical properties are related to size of an atom or how many protons/electrons it contains. For two elements diagonal to each other, they differ by one group (vertical column of periodic table) and share similar characteristics. Size decreases when you move from left to right, and increases w...
- Thu Nov 02, 2017 5:29 pm
- Forum: Lewis Structures
- Topic: Lewis Structures for Ions?
- Replies: 1
- Views: 336
Re: Lewis Structures for Ions?
Yeah, add or subtract the amount of electrons (add one electron for 1-, add two for 2-, remove one for 1+, remove 2 for 2+, etc.) then put your whole molecule in brackets [these things] and put the charge in the corner so ammonium would be [NH4]+ (except it would be nitrogen as the central atom with...
- Tue Oct 31, 2017 10:26 pm
- Forum: Trends in The Periodic Table
- Topic: Ionic Radii
- Replies: 2
- Views: 380
Re: Ionic Radii
With the loss of an electron, the remaining electrons in a cation are drawn closer to the nucleus. With the gain of an electron, the electron cloud of anions grows larger because electrons repel each other. Generally, increasing electrons (increasing negative charge) leads to increased ionic size an...
- Mon Oct 23, 2017 12:00 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: electron configuration for cation of Cr? [ENDORSED]
- Replies: 1
- Views: 252
Re: electron configuration for cation of Cr? [ENDORSED]
[Ar](3d^5)
You lose electrons from the largest number shell first (4th shell) here
and if you had even less electrons like it was Cr3+ then it would be [Ar](3d^3)
You lose electrons from the largest number shell first (4th shell) here
and if you had even less electrons like it was Cr3+ then it would be [Ar](3d^3)
- Mon Oct 23, 2017 11:23 am
- Forum: *Shrodinger Equation
- Topic: Double derivative [ENDORSED]
- Replies: 3
- Views: 729
Re: Double derivative [ENDORSED]
A double derivative is the same as a second derivative. Find the derivative of your function. Then, take another derivative -> you now have a double derivative.
- Mon Oct 23, 2017 11:20 am
- Forum: Administrative Questions and Class Announcements
- Topic: Where is BruinCast?
- Replies: 2
- Views: 361
Where is BruinCast?
Where can I find Bruincast for 14A? I know that they are on CCLE under the media tab but the CCLE links to Lavelle's website not the CCLE chem14A website... so anyone know where it is??
- Fri Oct 20, 2017 2:18 am
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Atomic Orbitals
- Replies: 2
- Views: 366
Re: Atomic Orbitals
Also the f orbital. So if the p orbital is two lobes, aka two ellipses, the d orbital would be (generally) like a double p with 4 lobes. And the f is (generally) like a triple p with 6 lobes (because one p has 2 lobes, so triple that would be 6 total). It's also arranged similarly, 6 ellipsoids orie...
- Fri Oct 20, 2017 2:07 am
- Forum: DeBroglie Equation
- Topic: Help with the concept of De Broglie's
- Replies: 8
- Views: 857
Re: Help with the concept of De Broglie's
Yeah, the wavelength exists but is very small and imperceivable. The entire concept of De Broglie's is to propose that all matter has wave-like properties, such as wavelengh. It is usually applied to describe the wave-like nature of an electron, but can still be used for larger objects. Just doesn't...
- Fri Oct 20, 2017 2:03 am
- Forum: DeBroglie Equation
- Topic: Homework Problems
- Replies: 3
- Views: 468
Re: Homework Problems
You can still turn in questions from chapter 1 as long as they're not the same as the ones you turned in last week. Since the email Lavelle sent out told us specifically which hw problems would be covered on the test, doing the hw from this section would be good preparation.
- Fri Oct 20, 2017 12:36 am
- Forum: DeBroglie Equation
- Topic: CHAPTER 1 QUESTION 33!!!
- Replies: 8
- Views: 1009
Re: CHAPTER 1 QUESTION 33!!!
Back to your original question, I understand it like this. You cannot use the Ek = 0.5mv^2=hc/lambda because we are calculating the wavelength for an electron, and there is a given velocity (3.6x10^3 km/s, in the problem) for this. Electrons don't travel at the speed of light (the constant c, in the...
- Fri Oct 13, 2017 1:30 am
- Forum: Limiting Reactant Calculations
- Topic: volume of stock solution needed to make 250ml of 0.650M NaOH
- Replies: 1
- Views: 2453
Re: volume of stock solution needed to make 250ml of 0.650M NaOH
If we used 250 mL of stock solution as you said, we would have 250 mL of 2.00 M NaOH. This is not what we want. What we want is 250 mL of 0.650 M NaOH. The stock solution is the solution calculated in Q2A. What you know about this stock is that it is 2.00 M NaOH, as given in the problem. So given th...
- Sun Oct 08, 2017 10:03 pm
- Forum: Properties of Light
- Topic: Chapter 1: Problem 9...Radiation from reading?
- Replies: 3
- Views: 501
Re: Chapter 1: Problem 9...Radiation from reading?
Yes, I think you're right. I mean, would you want to (or could you) read under either UV or infrared light rays? They aren't even visible to the human eye.
- Sun Oct 08, 2017 9:52 pm
- Forum: Limiting Reactant Calculations
- Topic: Limiting Reactant
- Replies: 9
- Views: 3044
Re: Limiting Reactant
When calculating for the limiting reactant, you need to not only find how many moles of each (cause usually you're given the reactants in grams of mass) you have, but how many moles of one reactant is needed in relation to the other reactants. For example, if your equation is X + 3Y -> 2Z then every...
- Fri Oct 06, 2017 9:46 pm
- Forum: Limiting Reactant Calculations
- Topic: Is either Method better?
- Replies: 4
- Views: 662
Re: Is either Method better?
Often, the problem will ask how much product is formed given two amounts of reactant. In this case, straight up calculating and comparing how much product would be formed from using all of each reactant would simultaneously give you the answer to how much product you actually get. Then, you can simp...
- Thu Oct 05, 2017 10:14 pm
- Forum: Administrative Questions and Class Announcements
- Topic: Question about pencils
- Replies: 1
- Views: 327
Question about pencils
I see that the syllabus says all tests and exams must be written in pen. But for the 4 HW problems that will be collected each week in the discussion, does anyone know if these can be done in pencil? I already did them in pencil, so I want to know if I have to transcribe them over to pen...