## Search found 38 matches

- Mon Mar 11, 2019 8:56 pm
- Forum: First Order Reactions
- Topic: 15.31 6th Edition
- Replies:
**3** - Views:
**37**

### Re: 15.31 6th Edition

Make sure the order of the reaction corresponds to the right half-life equation.

- Mon Mar 11, 2019 8:55 pm
- Forum: Arrhenius Equation, Activation Energies, Catalysts
- Topic: Arrhenius Equation.
- Replies:
**4** - Views:
**56**

### Re: Arrhenius Equation.

You use this equation when you either have activation energy or need to find it.

- Mon Mar 11, 2019 8:55 pm
- Forum: Reaction Mechanisms, Reaction Profiles
- Topic: 15.89
- Replies:
**1** - Views:
**22**

### 15.89

How would you draw a reaction profile for the reaction? Do we need to know how to do this?

- Tue Mar 05, 2019 2:26 pm
- Forum: First Order Reactions
- Topic: Integrating
- Replies:
**3** - Views:
**40**

### Re: Integrating

You should know how to get from the first equation to the last equation. Both of these will be given, but you should know how the last equation is derived from the first equation.

- Tue Mar 05, 2019 2:24 pm
- Forum: Phase Changes & Related Calculations
- Topic: Steam vs Boiling Water
- Replies:
**8** - Views:
**199**

### Re: Steam vs Boiling Water

Steam has a higher enthalpy because it takes more energy and heat to keep it as a gas. Therefore, it causes worse burns.

- Tue Mar 05, 2019 2:21 pm
- Forum: Method of Initial Rates (To Determine n and k)
- Topic: Zero, First, and Second Order reactions
- Replies:
**2** - Views:
**48**

### Re: Zero, First, and Second Order reactions

Yes, it is a second order reaction because the exponents that you multiply by in the rate equation add up to 2.

- Wed Feb 27, 2019 1:25 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: Entropy of Fusion
- Replies:
**3** - Views:
**61**

### Re: Entropy of Fusion

Yes, delta S can be both positive and negative.

- Wed Feb 27, 2019 1:23 pm
- Forum: Work, Gibbs Free Energy, Cell (Redox) Potentials
- Topic: flipping the sign of Ecell
- Replies:
**5** - Views:
**85**

### Re: flipping the sign of Ecell

All E cell values are reduction values. You can either flip the sign for oxidation or use the formula Ecell= Eright-Eleft

- Wed Feb 27, 2019 1:22 pm
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: Delta G at boiling point
- Replies:
**2** - Views:
**67**

### Re: Delta G at boiling point

It is 0 because water vaporizes at 100 degrees, therefore, the system is technically in equilibrium because the question asks for the delta g of vaporization.

- Sat Feb 23, 2019 4:13 pm
- Forum: Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams
- Topic: Cell Diagrams
- Replies:
**1** - Views:
**36**

### Cell Diagrams

On some of the homework solutions, they add a completely random element to the cell diagrams. For example, on 14.15, the cell diagram shows KOH, however there is no KOH in the solution. Can someone please explain?

- Thu Feb 21, 2019 3:10 pm
- Forum: Balancing Redox Reactions
- Topic: Finding Charge
- Replies:
**3** - Views:
**66**

### Re: Finding Charge

Use the charges from the periodic table! Hope this helps!

- Tue Feb 19, 2019 10:06 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: 9.81
- Replies:
**2** - Views:
**55**

### 9.81

Which is the thermodynamically more stable iron oxide in air, Fe3O4(s) or Fe2O3(s)? Justify your selection.

How do you know, is it based on the molecular mass?

How do you know, is it based on the molecular mass?

- Tue Feb 19, 2019 9:46 am
- Forum: Gibbs Free Energy Concepts and Calculations
- Topic: 9.69 in Sixth Edition
- Replies:
**1** - Views:
**49**

### 9.69 in Sixth Edition

What amount (in moles) of ATP could be formed if all the Gibbs free energy released in the oxidation of 3.00 mol NADH were used to generate ATP?

I do not know how to approach this problem given just three equations and delta G. Can anyone help me out?

I do not know how to approach this problem given just three equations and delta G. Can anyone help me out?

- Tue Feb 12, 2019 8:04 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: When is delta S = 0?
- Replies:
**3** - Views:
**312**

### Re: When is delta S = 0?

delta S equals zero when the reaction is reversible because entropy is a state function. When the process is reversible, it starts and ends in the same place making entropy equal to zero.

- Tue Feb 12, 2019 8:02 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Std Enthalpy of Formations
- Replies:
**1** - Views:
**33**

### Re: Std Enthalpy of Formations

Their heat of formation is zero because they are in their most stable state, that is why they are not included.

- Tue Feb 12, 2019 8:01 pm
- Forum: Entropy Changes Due to Changes in Volume and Temperature
- Topic: Extensive vs Intensive
- Replies:
**1** - Views:
**39**

### Re: Extensive vs Intensive

Heat capacity is extensive because it depends on the number of particles you have. Specific heat capacity and molar heat capacity are intensive because it is uniform for all molecules. For example, the specific heat of water is always 4.184 J/G x C and it does not matter how much water you have.

- Sat Feb 09, 2019 2:52 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: 9.35 Sixth Edition
- Replies:
**2** - Views:
**50**

### Re: 9.35 Sixth Edition

The book says container A has the most entropy, then C, then B.

- Sat Feb 09, 2019 2:30 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: 9.35 Sixth Edition
- Replies:
**2** - Views:
**50**

### 9.35 Sixth Edition

Container A is filled with 1.0 mol of the atoms of an ideal monatomic gas. Container B has 1.0 mol of atoms bound together as diatomic molecules that are not vibrationally active. Container C has 1.0 mol of atoms bound together as diatomic molecules that are vibrationally active. How do you determin...

- Fri Feb 08, 2019 11:58 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: Reaction Enthalpies
- Replies:
**2** - Views:
**49**

### Re: Reaction Enthalpies

I noticed the problems in the book have a distinct way they would prefer you to solve them. For example, to use the version where you break down the different reactions, the book gives you the equations. Hope this helps!

- Fri Feb 08, 2019 11:56 pm
- Forum: Calculating Work of Expansion
- Topic: Which P to use? 6th edition, 8.27
- Replies:
**3** - Views:
**69**

### Re: Which P to use? 6th edition, 8.27

Yes, the pressure you would use to find n is 1.79 atm.

- Fri Feb 08, 2019 11:51 pm
- Forum: Thermodynamic Definitions (isochoric/isometric, isothermal, isobaric)
- Topic: Work Equations
- Replies:
**2** - Views:
**56**

### Re: Work Equations

There is w=-PdeltaV, w=nRTln(V2/V1), and w=nRTln(P1/P2)

The first one would be used for constant pressure and irreversible reactions. The second and third ones would be used in isothermic reversible expansions.

The first one would be used for constant pressure and irreversible reactions. The second and third ones would be used in isothermic reversible expansions.

- Fri Feb 08, 2019 11:49 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: w=-PdeltaV
- Replies:
**6** - Views:
**100**

### Re: w=-PdeltaV

The first one is for reversible expansion, and the second one is for irreversible expansion.

- Sat Feb 02, 2019 9:29 pm
- Forum: Thermodynamic Systems (Open, Closed, Isolated)
- Topic: 8.31 Sixth Edition
- Replies:
**2** - Views:
**50**

### 8.31 Sixth Edition

Calculate the heat released by 5.025 g of Kr at .400 atm as it cools from 97.6 to 25.0 C at (a) a constant pressure and (b) constant volume.

I tried looking this up in the book and it wants to us to use fractions and stuff like that. Is there another way we learned how to do it in class?

I tried looking this up in the book and it wants to us to use fractions and stuff like that. Is there another way we learned how to do it in class?

- Thu Jan 31, 2019 5:13 pm
- Forum: Concepts & Calculations Using First Law of Thermodynamics
- Topic: 6th Edition, 8.9
- Replies:
**1** - Views:
**59**

### Re: 6th Edition, 8.9

You still use the 101.325 J to convert from L x atm to Joules. You should get -150.97 Joules for work and then convert it to kJ which is -.15 kJ, this is work. You then add work and q which is 5.5 kJ. Your final answer should be 5.35 kJ.

- Wed Jan 30, 2019 6:10 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Decreasing volume and chemical equilibrium
- Replies:
**8** - Views:
**142**

### Re: Decreasing volume and chemical equilibrium

When volume is decreased at equilibrium, the reaction will shift to the side with less moles. It also depends on how Q relates to K.

- Tue Jan 29, 2019 12:51 pm
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: 8.99 in Sixth Edition
- Replies:
**1** - Views:
**22**

### 8.99 in Sixth Edition

How would we go about finding the final temperature of HCl if the initial temperature is 25 degrees Celsius? What do you do with the volume and molarity you are given?

- Tue Jan 29, 2019 11:34 am
- Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
- Topic: Calorimeters
- Replies:
**3** - Views:
**59**

### Re: Calorimeters

We talked about it in lecture, so I'm assuming we need to know how to solve problems.

- Fri Jan 25, 2019 8:42 pm
- Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
- Topic: 8.3 6th Edition
- Replies:
**1** - Views:
**35**

### 8.3 6th Edition

I have no idea how to approach this problem. If somebody could please explain how to solve how much work is done, I would really appreciate it.

- Wed Jan 23, 2019 4:38 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: How to know when to use partial pressure or molar concentrations?
- Replies:
**4** - Views:
**83**

### Re: How to know when to use partial pressure or molar concentrations?

If they give Kp, convert it to atm or bar, but if it gives Kc leave it in terms of the molar concentration.

- Wed Jan 23, 2019 4:37 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Acids and Bases
- Replies:
**6** - Views:
**93**

### Re: Acids and Bases

You can also tell if it is an acid or base based on the equation. If it gives off OH-, then it is a base, and if it gives off H3O+, it is an acid.

- Wed Jan 16, 2019 8:40 pm
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: 7th Edition 5J.1
- Replies:
**3** - Views:
**49**

### Re: 7th Edition 5J.1

The concentration of H2 would increase because there is now more CO that is available to react. Also, the concentration of H2 would increase in order to keep the equilibrium constant the same.

- Wed Jan 16, 2019 8:39 pm
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: Acid and Base Equilibria
- Replies:
**7** - Views:
**106**

### Re: Acid and Base Equilibria

A weak acid has a higher pH. A pH of 7 is neutral, so the weaker the base, the closer to 7 it gets.

- Mon Jan 14, 2019 9:13 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: 12.23 in sixth edition
- Replies:
**1** - Views:
**48**

### 12.23 in sixth edition

I'm confused on how to set up the equation to get H30+ if we are only given one number which is Kw. Can someone please explain?

- Sat Jan 12, 2019 5:20 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE tables
- Replies:
**2** - Views:
**33**

### Re: ICE tables

When the coefficient is not equal to one you would simply add the coefficient in front of the x. For example if you had 2H2 you would subtract or add 2x.

- Wed Jan 09, 2019 9:23 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Calculating Kp
- Replies:
**2** - Views:
**24**

### Re: Calculating Kp

I believe you use the units that are given and you just use a constant that corresponds to the units that are given.

- Wed Jan 09, 2019 5:13 pm
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: 11.41 in 6th edition
- Replies:
**1** - Views:
**38**

### 11.41 in 6th edition

I was wondering how to set up the ICE table for this reaction. Do we have to convert into mol/L? Also do we assume that we start with no NH3 or CO2?

- Tue Jan 08, 2019 4:21 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Concentrations of products/reactants
- Replies:
**6** - Views:
**80**

### Re: Concentrations of products/reactants

Q would be anything other than equilibrium, and K is the equilibrium.

- Tue Jan 08, 2019 11:23 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: 11.37 6th Edition
- Replies:
**3** - Views:
**69**

### 11.37 6th Edition

I was wondering if anyone could explain how to find the partial pressures of N2, H2, and NH3 when only given that K=41. Do we have to involve constants from a table?