## Search found 55 matches

Sun Mar 15, 2020 4:27 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Redox from cell diagram
Replies: 6
Views: 169

### Re: Redox from cell diagram

The commas are used just because they the two molecules are in the same phase, but other than that, the molecule is being reduced.
Sun Mar 15, 2020 4:25 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Replies: 8
Views: 187

### Re: adding platinum

Also, hydrogen electrodes need an inert metal such as platinum.
Sun Mar 15, 2020 4:21 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: electrodes
Replies: 3
Views: 143

### Re: electrodes

Is it safe to assume the hydrogen cell will be the anode because when calculating E cell standard, any positive number minus 0 will give a postive voltage?
Sun Mar 15, 2020 4:17 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: Flipping the anode
Replies: 4
Views: 139

### Re: Flipping the anode

Flipping the anode identifies it as an oxidation reaction and allows us to cancels out the electrons with the cathode side when writing the equation.
Sun Mar 15, 2020 4:14 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: nernst
Replies: 5
Views: 164

### Re: nernst

When using the equation delta g = -nFe, e cell doesn't change and G does because of the n which is number of electrons transferred. Doubling the equation means increasing the number of electrons changing the value of G.
Sun Mar 15, 2020 4:12 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: lnQ
Replies: 12
Views: 171

### Re: lnQ

Yes, and also make sure you write out the chemical reaction to find out which are the products and the reactants. Q = products/reactants.
Sun Mar 15, 2020 4:08 pm
Forum: Appications of the Nernst Equation (e.g., Concentration Cells, Non-Standard Cell Potentials, Calculating Equilibrium Constants and pH)
Topic: Test 2 Q6 part b ii
Replies: 5
Views: 151

### Re: Test 2 Q6 part b ii

In addition, if you look at the equation for it, mass isn't accounted for anywhere.
Sun Mar 15, 2020 3:59 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Affecting E cell
Replies: 4
Views: 148

### Affecting E cell

How does changing concentration of reactants or products in a reaction effect E cell?
Sun Mar 15, 2020 3:57 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Cell Diagram
Replies: 11
Views: 224

### Re: Cell Diagram

If we have two molecules that are both solid, do we still have to use Pt or any other inert metal since they are in the same phase.
Sun Mar 15, 2020 3:55 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: SHE
Replies: 3
Views: 122

### Re: SHE

Also remember, when writing the cell diagram to add Pt or any other inert metal.
Sun Mar 15, 2020 3:52 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Galvanic and voltaic cells
Replies: 5
Views: 173

### Re: Galvanic and voltaic cells

They are the same. The difference comes when comparing them to electrolytic cell. A galvanic cell transforms chemical energy into electrical energy. An electrolytic cell converts electrical energy into chemical energy.
Sun Mar 15, 2020 3:50 pm
Forum: Balancing Redox Reactions
Topic: Half rxns
Replies: 27
Views: 576

### Re: Half rxns

To the question : "Do you always add the H2O at opposite ends of where you have added OH or H+?"

You should be adding the h20 first and then adding OH or the H to the opposite side to balance the number of hydrogens.
Sun Mar 15, 2020 3:47 pm
Forum: Balancing Redox Reactions
Topic: Half rxns
Replies: 27
Views: 576

### Re: Half rxns

I believe the side that has less hydrogens is the side you would add the OH because the purpose of adding it is to balance the number of hydrogen and this is only in basic solutions
Sun Mar 15, 2020 3:44 pm
Forum: Balancing Redox Reactions
Topic: Oxidation/Reduction
Replies: 17
Views: 402

### Re: Oxidation/Reduction

To add on, the reducing agent is basically the molecules getting oxidized because it releases the electron that is added and reducing the other molecule. In the same sense, the oxidizing agent is the molecules getting reduced.
Sun Mar 15, 2020 3:40 pm
Forum: Balancing Redox Reactions
Topic: Ecell values
Replies: 12
Views: 281

### Re: Ecell values

In addition to the answers given, the reason we want to have a positive E cell is because it leads to a negative standard gibbs free energy which in turn means a positive value for entropy meaning the process is spontaneous.
Sun Mar 15, 2020 3:35 pm
Forum: Balancing Redox Reactions
Topic: changing half reactions
Replies: 6
Views: 168

### Re: changing half reactions

In the anode, usually the reverse of the given half reactions is occuring, because oxidation has to take place in the anode, right?
Sun Mar 15, 2020 3:31 pm
Forum: Balancing Redox Reactions
Topic: Pt in Cell Diagram
Replies: 14
Views: 307

### Re: Pt in Cell Diagram

Also, pt is used when dealing with hydrogen, and when two of the molecules are in the same phase such as both are aqueous solutions.
Mon Mar 09, 2020 1:05 am
Forum: General Rate Laws
Topic: Making one reactant concentration small
Replies: 3
Views: 83

### Re: Making one reactant concentration small

I think making of the reaction concentration smaller conceptually simulates the reactant not having as much of an affect on reaction rate allowing us to see kind of affect the other reactant has.
Mon Mar 09, 2020 12:58 am
Forum: General Rate Laws
Topic: Enzyme saturation
Replies: 6
Views: 93

### Re: Enzyme saturation

When enzyme is saturated, the increase in reaction rate levels off.
Mon Mar 09, 2020 12:56 am
Forum: General Rate Laws
Topic: Difference between each order of reaction
Replies: 3
Views: 109

### Re: Difference between each order of reaction

zero order reaction occurs at a constant rate. First order reaction rate is dependent on a reactant concentration and second order reaction rate is dependent on the square of a concentration of reactant.
Mon Mar 09, 2020 12:53 am
Forum: General Rate Laws
Topic: Second order reaction
Replies: 1
Views: 1135

### Second order reaction

What is relationship between the half life of the second order reaction and the concentration of the reactant?
Mon Mar 09, 2020 12:45 am
Forum: General Rate Laws
Topic: Integrated Rate Laws
Replies: 3
Views: 77

### Re: Integrated Rate Laws

It gives the concentration of reactants or products at anytime after the start of the reaction.
Mon Mar 02, 2020 6:07 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: 6L.3 e
Replies: 1
Views: 24

### 6L.3 e

for 6L.3 part e, the for the half reaction in the anode the solutions manual says
Sn4+ + 2e- --> Sn2+, but the book problem doesn't show Sn2+, just Sn2 so aren't we supposed to assume it is two molecules of Sn instead a charge of 2+ so the balanced equation should be 2Sn4+ + 8e- -->Sn2?
Sun Mar 01, 2020 10:50 pm
Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
Topic: Free Energy and Cell Potential Relationship
Replies: 3
Views: 96

### Re: Free Energy and Cell Potential Relationship

They are related through the equation deltaG = -nF(deltaE). G is Gibbs free energy, n is number of electrons transferred, F is faraday constant, and e is cell potential. If cell potential is negative then reaction is spontaneous and if it is positive then reaction is non spontaneous.
Sun Mar 01, 2020 10:42 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Cathode/Right & Anode/Left
Replies: 7
Views: 96

### Re: Cathode/Right & Anode/Left

To add on, the electrode at which the electrons enter and “add to” the cell is the cathode while the electrode at which the electrons leave the cell is the anode.
Sun Mar 01, 2020 10:38 pm
Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
Topic: Degree symbol
Replies: 10
Views: 138

### Re: Degree symbol

The degree symbol indicates standard conditions for the process while without the degrees indicates whatever conditions the reaction is given in.
Sun Mar 01, 2020 10:24 pm
Forum: Balancing Redox Reactions
Topic: Reducing Agent
Replies: 5
Views: 131

### Reducing Agent

In a reaction, the reducing agent is the one that is oxidized and the oxidizing agent is the one that is reduced, right?
Sun Mar 01, 2020 10:21 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Galvanic and Voltaic Cells
Replies: 7
Views: 121

### Re: Galvanic and Voltaic Cells

They are the same. The difference is between electrochemical cells and galvanic cells. I believe electrochemical cells convert electrical energy into chemical energy while galvanic cells convert chemical energy into electrical energy.
Sun Feb 23, 2020 11:14 pm
Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
Topic: G(not) and G
Replies: 15
Views: 260

### Re: G(not) and G

Isn't the equation G = Gnot + RTlnQ ?
Sun Feb 23, 2020 10:58 pm
Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
Topic: Vant Hoff Equation
Replies: 9
Views: 185

### Re: Vant Hoff Equation

The Vant Hoff equation can also be manipulated and use to calculate K at a different temperature if delta H is known.
Sun Feb 23, 2020 10:46 pm
Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
Topic: Porous disk
Replies: 3
Views: 42

### Re: Porous disk

I think there should still be separation of the half reactions as long there is a method for the transport of ions or electrons
Sun Feb 23, 2020 10:45 pm
Forum: Balancing Redox Reactions
Topic: Potential Difference
Replies: 5
Views: 141

### Potential Difference

Can someone explain what is meant by potential difference?
Thu Feb 20, 2020 2:09 pm
Forum: Gibbs Free Energy Concepts and Calculations
Topic: 5G.15
Replies: 5
Views: 114

### 5G.15

for 5G.15 I keep getting -2.7 kj per mol but the answer says -27 kj per mol. Can someone tell me what I'm doing wrong is the answer key wrong.
Sun Feb 16, 2020 11:13 pm
Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
Topic: Reversible vs Irreversible
Replies: 5
Views: 182

### Re: Reversible vs Irreversible

Irreversible processes are usually spontaneous and quick where as irreversible processes are slow and maintain equilibrium throughout the entirety of the process. However, I believe it will be clearly stated or inferred in any test.
Sun Feb 16, 2020 11:08 pm
Forum: Calculating Standard Reaction Entropies (e.g. , Using Standard Molar Entropies)
Topic: What is residual entropy?
Replies: 14
Views: 2033

### Re: What is residual entropy?

Yes, positional entropy is a result of change in volume, for example where a gas expands in a larger volume, while residual entropy is I believe a result of dipole dipole interactions.
Sun Feb 16, 2020 11:04 pm
Forum: Concepts & Calculations Using Second Law of Thermodynamics
Topic: spontaneity
Replies: 39
Views: 827

### Re: spontaneity

To add on, when Gibbs free energy is negative that means that according the equation for gibbs free energy, delta S or change in entropy is positive and if change in entropy is positive, it means that a process is spontaneous.
Sun Feb 16, 2020 10:58 pm
Forum: Gibbs Free Energy Concepts and Calculations
Topic: Delta H
Replies: 1
Views: 56

### Delta H

I forgot what Dr. Lavelle said in lecture, but it was something about delta H or the change in enthalpy doesn't change even if temperature changes? Can someone explain exactly what he said and what it means?
Sun Feb 16, 2020 10:47 pm
Forum: Van't Hoff Equation
Topic: Van't Hoff Equation
Replies: 3
Views: 110

### Re: Van't Hoff Equation

The equation is used to find out the change in the equilibrium constant, K, of a chemical reaction with the change in temperature and standard enthalpy change.
Mon Feb 03, 2020 9:41 pm
Forum: Phase Changes & Related Calculations
Topic: -w vs w
Replies: 15
Views: 206

### Re: -w vs w

When w is negative, it means that the system is doing work, while when w is positive, it means that the system is having work done on it.
Sun Feb 02, 2020 10:41 pm
Forum: Phase Changes & Related Calculations
Topic: enthalpy change
Replies: 2
Views: 76

### enthalpy change

Is enthalpy change for a reverse reaction the negative of the enthalpy change for the forward reaction?
Sun Feb 02, 2020 10:29 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: Volume and enthalpy
Replies: 1
Views: 43

### Volume and enthalpy

If the volume stayed constant, could change in enthalpy still be equal to heat added?
Sun Feb 02, 2020 10:03 pm
Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
Topic: Reaction constant P
Replies: 3
Views: 36

### Re: Reaction constant P

Gases can change volume depending on pressure but solids and liquids maintain a constant volume.
Sun Feb 02, 2020 9:52 pm
Forum: Phase Changes & Related Calculations
Topic: Reversible and Irreversible
Replies: 5
Views: 68

### Re: Reversible and Irreversible

Also, irreversible processes almost always do more work than reversible processes.
Sun Feb 02, 2020 9:44 pm
Forum: Thermodynamic Systems (Open, Closed, Isolated)
Topic: Isolated system
Replies: 10
Views: 252

### Re: Isolated system

A system is considered isolated when the system cannot exchange energy/heat with its surroundings. An example would be a boiling water in a closed insulated container, like a hydroflask. This is considered an isolated system because the hot water in the container cannot exchange heat/energy with the...
Sun Jan 26, 2020 10:45 pm
Forum: Phase Changes & Related Calculations
Topic: State functions
Replies: 3
Views: 31

### State functions

So heat isn't a state function but internal energy of an isolated system is a state function. What qualifies something to be, or not to be, a state function?
Sun Jan 26, 2020 10:32 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: Exothermic and Endothermic
Replies: 11
Views: 439

### Re: Exothermic and Endothermic

Exothermic is negative because it is releasing energy, while endothermic is positive because it is absorbing energy
Sun Jan 26, 2020 10:23 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: 3 methods
Replies: 5
Views: 48

### Re: 3 methods

You should use certain methods based on the information you are given, so different methods for different circumstances, but also I believe that the methods using bond enthalpies is the least accurate method because the bond enthalpies of non-diatomic molecules are averages from many different molec...
Sun Jan 26, 2020 10:13 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: Different Enthalpy Strategies
Replies: 5
Views: 52

### Re: Different Enthalpy Strategies

If I remember correctly, using the strategy with the bond enthalpies is the least accurate method so there is a benefit to using the other two.
Sun Jan 26, 2020 10:05 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: The 3 methods
Replies: 4
Views: 59

### The 3 methods

I forgot to write it in my notes, but which of the three methods was supposed to be the least accurate?
Sun Jan 19, 2020 10:23 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Textbook clarification: weak acids and bases
Replies: 3
Views: 50

### Re: Textbook clarification: weak acids and bases

OH- are the conjugate base of water. However, if water reacts with an acid, wouldn't it act as a base thus it would have a conjugate acid of hydronium ions?
Sun Jan 19, 2020 10:13 pm
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: pKa
Replies: 13
Views: 115

### Re: pKa

pKa = -log Ka; so according to that equation, the lower the pKa is, the higher the Ka will be meaning it is a stronger acid. The higher the pKa is, the lower the Ka will be meaning it will be a weaker acid.
Tue Jan 14, 2020 11:12 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: 5H.2
Replies: 2
Views: 57

### 5H.2

So for problem 5H.2, the book says that for the reaction, K = 2.5 * 10^10, however in the solutions manual they use K = 2.5 * 10^7 for the calculations. Can someone please explain? Am I missing something here?
Sun Jan 12, 2020 11:24 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Homogenous Equilibrium
Replies: 13
Views: 116

### Re: Homogenous Equilibrium

It is homogeneous when the products and reactants are in the same phase. Heterogeneous is when the all the products and reactants aren't in the same phase so you would have to omit pure liquids and solids in your equilibrium calculations.
Sun Jan 12, 2020 11:12 pm
Forum: Equilibrium Constants & Calculating Concentrations
Topic: Calculating K
Replies: 9
Views: 79

### Re: Calculating K

pure liquids and solids, which includes water, are disregarded for the equilibrium expression because they don't have an affect on reactant amount at equilibrium and they don't have a concentrations to be used to calculate k.
Sun Jan 12, 2020 11:03 pm
Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
Topic: pressure and volume
Replies: 4
Views: 40

### Re: pressure and volume

When you look at the ideal gas , pv=nrt, the numbers have to be constant, so if p is being doubled v has to be halved since they are being multiplied to balance out and keep the value of nrt constant.

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