CHEMISTRY COMMUNITY

Helen Zhao 1F

For Question 7, I wrote out an equation and balanced it out. I got CH4 + 2O2 -> 2H2O + CO2. I then drew out diagrams for each molecule and calculated the delta H for each. CH4 was 1648kJ, O2 was 992kJ, H2O was 1852 kJ, and CO2 was 1486kJ. I finally did (delta H of CH4 + O2) - (delta H of H2O + CO2) ...

Helen Zhao 1F

For Question 6, I first found delta V using (delta)nRT/P. Using delta V, I plugged the values given into delta U = delta H -PdeltaV. delta H = 4 * -2878 kJ/mol and PdeltaV = (-1atm)(282L)(8.314 J/Kmol )(1/8.206*10^-2Latm/Kmol)(1kJ/1000J) = 28.6kJ. Using those values I got -11541 kJ.

Helen Zhao 1F

I used the pKa to find pKb.
I used pKb to find Kb.
I then made an ice table and used that to find the concentration of OH-.
I used the concentration of OH- to find the pOH.
Finally, I used pOH to convert to pH.

Helen Zhao 1F

For part A of question 15.39 from the 6th edition, how does the coefficient in front of the reactant affect the equation? If it was just A -> B + C would it still be the same answer?

Helen Zhao 1F

For 15.17 from the 6th edition, why did we use the 2nd and 4th experiment to find the order of A? Why couldn't we use the 1st and 2nd or 3rd and 4th? And how do we know C is independent from the rate.

Helen Zhao 1F

During Lavelle's lecture today, why was there a 1/2 in front of dNO2/dt in step 2?

Helen Zhao 1F

During the lecture today, why did k = 2k2K = 2k1k2/k'1? I don't get how he derived this formula.

Helen Zhao 1F

delta G equals to 0 when the equation is at equilibrium. At equilibrium, the amount of energy released by reactants is used by the products or vice versa. As a result, there is no change in free energy because all the energy released is absorbed.

Helen Zhao 1F

Based on Lavelle's sig fig sheet, integers and exact numbers do not affect sig figs.

Helen Zhao 1F

Under what circumstance would you include Pt in the cell diagram and when do you not include it?

Helen Zhao 1F

For question 9.65 from the 6th edition, how do you know if the compound is decomposing for forming. For example, how do you know its P + 5/2Cl2 -> PCL5 instead of PCl5 -> P + 5/2Cl2?

Helen Zhao 1F

When you balance the equations for 9.65 in the 6th edition, why are the balanced coefficients in fractions?

Helen Zhao 1F

For question 14.15a, how do you which equation is the cathode or anode?

Helen Zhao 1F

The equilibrium constant only applies for gases therefore solids and liquids are disregarded.

Helen Zhao 1F

If you were given the specific heat capacity I would use the given value but it should equal 5/2 R if pressure is constant and 3/2R if volume is constant.

Helen Zhao 1F

In a calorimeter, no heat is lost to the surroundings so the heat released from the reaction is absorbed by the calorimeter. q reaction is negative because heat is lost and q calorimeter is positive because heat is absorbed.

Helen Zhao 1F

The human body as a whole would be considered an open system.

Helen Zhao 1F

In a spontaneous reaction, enthalpy is negative, entropy is positive and Gibbs Free Energy is negative. In a nonspontaneous reaction, enthalpy is positive, entropy is negative and Gibbs Free Energy is positive.

Helen Zhao 1F

For problem 4F.3 from the 7th edition, why is there a greater change of entropy at a lower temperature?

Helen Zhao 1F

Bond formation is exothermic. Energy is released when bonds are formed. When a new bond is formed, there is a net lowering of energy and heat is released into the environment. It costs energy to break a bond so bond breaking is endothermic.

Helen Zhao 1F

It is J/C*mol because C-1 = 1/C and mol-1 = 1/mol.

Helen Zhao 1F

Specific heat capacity is the amount of heat needed to raise the temperature of an object per unit mass of an object. In other words, specific heat capacity is the heat capacity per unit mass of a material.

Helen Zhao 1F

When you freeze something, the heat from the object is absorbed into the surroundings and as a result, the total heat in the system is lost. When heat is lost, enthalpy becomes more negative. When you melt something, heat is added into the object and the total heat of the system is increased. Enthal...

Helen Zhao 1F

Enthalpy is the total energy in the system. The reactants require energy to break the bonds so the sign is positive when energy goes into the system and because energy is released when bonds form in the products, energy goes out and the sign is negative.

Helen Zhao 1F

Enthalpy is the amount of heat released or absorbed at constant pressure. Whether or not it's kJ or kJ * mol^-1, it doesn't really matter. Just remember to use the units that best fits the question asked.

Helen Zhao 1F

They're all bases because the question says "given that the pka of its conjugate acid". "its" refers to the molecules listed in each subsection (a, b, c, d) and because the question says conjugate acid, then "its" are bases.

Helen Zhao 1F

But because there is an equal number moles of gases on each side of the reaction, compressing the system should have little to no effect.

Helen Zhao 1F

The larger the pKa the weaker the acid.

Helen Zhao 1F

This statement is true because the concentration of the reactants over the products at equilibrium should equal the equilibrium constant. The constant for the reaction at equilibrium will not change, therefore, as you increase the concentration of the reactants, the concentration of the products sho...

Helen Zhao 1F

To find k you use the concentrations of the products and the reactants. The reason there isn't any units is because concentrations are an approximation of chemical activity and chemical activity does not have any units. We use concentration instead of chemical activity because chemical activity is t...

Helen Zhao 1F

For Question 11.3 from the 6th edition textbook, the question asks to find the equilibrium constant of the following equations. According to the solution manual, the equilibrium constant involves the partial pressure of the molecules. Is it partial pressure because we do not know the molarity of the...

CHEMISTRY COMMUNITY

Search found 31 matches

Re: Midterm Question 6

Re: Midterm Question 6

Re: Test 1 problem 5

6th edition 15.39

6th edition 15.17

1/2 dNO2/dt

k in Lavelle's Lecture

Re: delta G = 0 ??

Re: Significant Figures

Pt

9.65 6th edition writing chemical equations

9.65 6th edition

14.15 a 6th edition

Re: Liquid and moles

Re: Ideal gases

Re: 6th edition 8.25

Re: Structures of the Human Body and Systems

Re: enthalpy, entropy, Gibbs Free Energy signs

Change in entropy and its relation with temperature

Re: Bond Formation

Re: Units

Re: Heat Capacity vs. Specific Heat Capacity

Re: Phase change enthalpy signs

Re: Signs in bond enthalpies

Re: Enthalpy Units

Re: 6th Edition 12.59

Re: Number 115 Chapter 11 HW

Re: Pka and Acidty

Re: Question 5G.1 part d

Re: Equilibrium constant

Homework Problem 11.3 for 6th Edition