Search found 43 matches
- Fri Mar 16, 2018 11:15 pm
- Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
- Topic: Question 14.41
- Replies: 6
- Views: 998
Re: Question 14.41
WHat's this about concentration?
- Fri Mar 16, 2018 11:00 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: closed vs isolated
- Replies: 11
- Views: 1380
Re: closed vs isolated
Does heat transfer happen when the balloon loses air?
- Fri Mar 16, 2018 10:59 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Catalysts
- Replies: 2
- Views: 356
Re: Catalysts
They orient the molecules in a way that makes them easier to crash in the correct orientation.
- Fri Mar 16, 2018 10:59 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagram
- Replies: 3
- Views: 479
Re: Cell Diagram
Is the salt bridge also connected to, say, Pt(s)? or just metal wire?
- Thu Mar 15, 2018 6:38 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Test 2 #6
- Replies: 3
- Views: 483
Re: Test 2 #6
You can tell because of the cell potentials. Overall cell potential has to be positive.
- Thu Mar 15, 2018 6:35 pm
- Forum: *Electrophilic Addition
- Topic: Possible Questions
- Replies: 1
- Views: 1168
Re: Possible Questions
Questions like which?
- Thu Mar 15, 2018 6:34 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 15.49
- Replies: 4
- Views: 681
Re: 15.49
Yes rate law is only the slow step
- Thu Mar 15, 2018 6:33 pm
- Forum: Balancing Redox Reactions
- Topic: Half-Reactions Sheet
- Replies: 5
- Views: 743
- Fri Mar 09, 2018 2:20 pm
- Forum: Second Order Reactions
- Topic: Units [ENDORSED]
- Replies: 5
- Views: 858
Re: Units [ENDORSED]
What about units for a 1.5 order?
- Fri Mar 09, 2018 2:19 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Rate Constant Calculations [ENDORSED]
- Replies: 3
- Views: 604
Re: Rate Constant Calculations [ENDORSED]
You could use the linear equations for the standard rxn numbers to find the constant from initial and time concentrations
- Fri Mar 09, 2018 2:18 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Finding n
- Replies: 15
- Views: 1890
Re: Finding n
But if you multiply entire reaction by 2 then why isn’t it using 2 moles?
- Sat Mar 03, 2018 10:41 pm
- Forum: Second Order Reactions
- Topic: K in Rate Laws [ENDORSED]
- Replies: 2
- Views: 434
Re: K in Rate Laws [ENDORSED]
Because for second order reactions the y-axis is 1/[A]. As time progresses the concentration of [A] decreases (assuming A is reactant) and thus 1/A increases, therefore slope of graph >0
- Sat Mar 03, 2018 10:39 pm
- Forum: General Rate Laws
- Topic: Multiple Reactants
- Replies: 2
- Views: 362
Re: Multiple Reactants
1) Double reaction and initial rates are doubled: let's pretend A --> B, [A] = c mol/L and rate = k [A]^1. Your rate would be k*c^1 = kc But let's say [A] = 2c, then rate would be k*(2c)^1 = 2kc So for first order with respect to a reactant, doubling the concentration would give you double the rate
- Sat Mar 03, 2018 10:37 pm
- Forum: First Order Reactions
- Topic: Reaction Orders [ENDORSED]
- Replies: 2
- Views: 420
Re: Reaction Orders [ENDORSED]
They basically mean, in crass terms, "How much does the concentration of reactant affect rate of reaction"
- Sun Feb 25, 2018 4:24 pm
- Forum: Zero Order Reactions
- Topic: zero order slopes
- Replies: 5
- Views: 858
Re: zero order slopes
Yes, slope should be zero. It's the derivative of a constant, which makes it zero.
- Sun Feb 25, 2018 4:23 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Finding n
- Replies: 15
- Views: 1890
Re: Finding n
How do we know it's a mole of reaction?
- Sun Feb 25, 2018 4:23 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Determining N
- Replies: 4
- Views: 628
Re: Determining N
Determined by the balanced equation or no?
- Tue Feb 20, 2018 10:01 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: 14.27
- Replies: 1
- Views: 284
Re: 14.27
Yes i believe so. Thanks for the tip. Got stuck on this one
- Fri Feb 16, 2018 5:18 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Anode/ Cathode
- Replies: 6
- Views: 829
Re: Anode/ Cathode
Red Cat-- reduction at cathode
An Ox-- anode oxidation
An Ox-- anode oxidation
- Fri Feb 16, 2018 5:17 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: s vs. delta s
- Replies: 7
- Views: 1732
Re: s vs. delta s
I thought we can only measure change in entropy?
- Fri Feb 16, 2018 5:16 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: What does R stand for?
- Replies: 13
- Views: 3402
Re: What does R stand for?
Yes, you're right sorry. THere's multiple R. You need to look at the units, on the third row of equation sheet. THanks
- Sat Feb 10, 2018 3:08 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: closed vs isolated
- Replies: 11
- Views: 1380
Re: closed vs isolated
No, closed is just where matter can't escape. isolated is where neither matter nor internal energy can escape
- Sat Feb 10, 2018 3:06 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: finding heat capacity using q=cΔT
- Replies: 3
- Views: 1053
Re: finding heat capacity using q=cΔT
The heat capacity is defined as ENERGY per TEMPERATURE
- Sat Feb 10, 2018 3:04 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: When to use + sign
- Replies: 11
- Views: 1072
Re: When to use + sign
So since it's for a change its always used?
- Sat Jan 27, 2018 8:33 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: Examples of work being done
- Replies: 7
- Views: 1014
Re: Examples of work being done
For example pushing a cart is work being done. You use some energy (instead of to heat up) to push the cart.
- Sat Jan 27, 2018 8:31 pm
- Forum: Concepts & Calculations Using Second Law of Thermodynamics
- Topic: Entropy of gas vs liquid vs solid
- Replies: 7
- Views: 8940
Re: Entropy of gas vs liquid vs solid
Because gas has more "randomness" by intuition. THere is inherently order in a liquid and solid-- they are all contained and there is only a set place that they can go. Gravity dictates this in a liquid and the lattice of a solid dictates this
- Sat Jan 27, 2018 8:29 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: units for delta H
- Replies: 4
- Views: 667
Re: units for delta H
KJ, or KJ per mole. depends on the context.
- Sat Jan 20, 2018 10:54 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: What does R stand for?
- Replies: 13
- Views: 3402
Re: What does R stand for?
Heat constant. When do you use 8.314 and when do you use 0.00821?
- Sat Jan 20, 2018 10:54 am
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: Calorimeter
- Replies: 10
- Views: 1075
Re: Calorimeter
The calorimeter is usually calibrated well so that there is little heat lost that is not absorbed by the substance you are measuring heat. Thus you can measure the heat of a reaction, and thus you can also measure the heat per mole (by measuring the amt. of substance consumed)
- Sat Jan 20, 2018 10:52 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy
- Replies: 4
- Views: 445
Re: Enthalpy
Bond enthalpy is equal to enthalpy of formation in a diatomic molecule; for the others it is the sum of the bond enthalpies i believe. Correct me if wrong
- Fri Jan 12, 2018 10:29 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Enthalpy Change Signs
- Replies: 5
- Views: 1448
Re: Enthalpy Change Signs
Think of it as enthalpy of formation being the same for each substance no matter whether it is on reactant or product side. Thus, if reactants - products = H, products - reactants = -H
- Fri Jan 12, 2018 10:26 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Why is fusion another name for melting?
- Replies: 4
- Views: 461
Re: Why is fusion another name for melting?
You might also be able to think of it as fusion being the heat it takes to put together, which is the reverse and equal in absolute value to the heat it takes to break apart?
- Fri Jan 12, 2018 10:24 am
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Bond Enthalpies vs. Standard Enthalpies of Formation
- Replies: 2
- Views: 216
Re: Bond Enthalpies vs. Standard Enthalpies of Formation
Is standard enthalpy of formation based on forming from the gaseous state as well?
- Wed Nov 30, 2016 1:24 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Calculating pH of a weak acid and its salt
- Replies: 1
- Views: 584
Re: Calculating pH of a weak acid and its salt
KNO2 has NO2- when it dissociates, which it will because any compound with K+ will dissociate (generally).
Therefore, we have an initial concentration of NO2- to plug into ICE box
Therefore, we have an initial concentration of NO2- to plug into ICE box
- Wed Nov 30, 2016 1:23 pm
- Forum: *Titrations & Titration Calculations
- Topic: Titrations
- Replies: 1
- Views: 478
Re: Titrations
Why do we want strong base/strong acid to be the titrant?
- Wed Nov 30, 2016 1:22 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 12.57, pH/pOH v. pKa/pKb
- Replies: 1
- Views: 619
Re: 12.57, pH/pOH v. pKa/pKb
No, pH is the measure of the [H+], while pKa is the measure of basically how much of a given acid HA dissociates. They are related, though. While Ka value doesn't tell too much about H+ concentration (due to other things like diprotonations, 2 H+ / mol acid), if everything else is held constant, suc...
- Sat Nov 26, 2016 6:01 pm
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Can you classify acids as strong or weak from their formulas alone? [ENDORSED]
- Replies: 7
- Views: 1749
Re: Can you classify acids as strong or weak from their formulas alone? [ENDORSED]
No, usually not. The only strong acids are the ones that are listed as "strong acids," and we know this because a Ka value doesn't exist-- everything dissociates so [HA] == 0, and Ka becomes undefined. Theoretically, you could deduce based on electronegativity its ionic vs covalent charact...
- Mon Nov 14, 2016 1:37 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Equilibrium Concentration Units [ENDORSED]
- Replies: 3
- Views: 1654
Re: Equilibrium Concentration Units [ENDORSED]
Just molarity, since all units are the same, and some have varying degrees, so it wouldnt make sense to have units.
- Thu Oct 27, 2016 3:07 pm
- Forum: Ionic & Covalent Bonds
- Topic: Determining Which Has A Stronger Bond
- Replies: 2
- Views: 1719
Re: Determining Which Has A Stronger Bond
Bonds work because of a balance of attraction between electrons and protons, and that they're not so close that the protons in the nucleus repel each other. Therefore, shorter bonds are better because the protons can easier "grab" the electrons.
- Fri Oct 21, 2016 11:47 am
- Forum: Trends in The Periodic Table
- Topic: What is the difference between electron affinity and electronegativity?
- Replies: 3
- Views: 992
Re: What is the difference between electron affinity and electronegativity?
They are inversely related-- electron affinity is the energy required to eject an electron, while electronegativity is the tendency to gain an electron
- Fri Oct 14, 2016 1:27 am
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Rydberg Equation [ENDORSED]
- Replies: 4
- Views: 1074
Re: Rydberg Equation [ENDORSED]
Will we be given that it is a hydrogen atom? This only works for hydrogen, but the problem 8 in the practice quiz 2 didn't list it as a hydrogen atom.
- Thu Oct 06, 2016 8:32 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Boundary Surface of Orbitals [ENDORSED]
- Replies: 2
- Views: 1587
Re: Boundary Surface of Orbitals [ENDORSED]
Those shapes are right, but important to note that it's not the "boundary," but rather the probability region-- where an electron is most likely to be-- if I understand correctly!
- Thu Sep 29, 2016 2:11 am
- Forum: Trends in The Periodic Table
- Topic: Electron Affinity [ENDORSED]
- Replies: 3
- Views: 667
Re: Electron Affinity [ENDORSED]
I believe nitrogen has an electron affinity so much lower because it has (relatively) much fewer protons than oxygen and fluorine. Also what Alexis said about stability and all orbitals being half-filled: most stable when either all half-filled or all filled