AP Chemistry : Thermodynamics
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Example Questions
Example Question #1 : Hess' Law
Using the following data to calculate the enthalpy change in: C4H10O(l) -> C4H8 (g) + H2O (g)
152 kJ/mol
-152 kJ/mol
-17 kJ/mol
76 kJ/mol
-76 kJ/mol
76 kJ/mol
Example Question #2 : Hess' Law
Using the following data to calculate the enthalpy change in: CaO (s) + H2O (l) -> Ca(OH)2 (aq)
147 kJ/mol
-62 kJ/mol
124 kJ/mol
-124 kJ/mol
-147 kJ/mol
-147 kJ/mol
Example Question #3 : Hess' Law
Using the following data to calculate the enthalpy change in: B2H6 (g) + 3 O2 (g) -> B2O3 (s) + 3 H2O (l)
2168 kJ/mol
-1084 kJ/mol
1084 kJ/mol
-2168 kJ/mol
3252 kJ/mol
-2168 kJ/mol
Example Question #121 : Thermochemistry And Kinetics
Consider an electrochemical cell that has the following overall reaction:
2 H+(aq) + Sn (s) -> Sn2+ (aq) + H2 (aq)
Which of the following changes would alter the measured cell potential?
Increase the pH in the cathode.
Increasing the H2 pressure in the cathode.
Lowering the pH in the cathode.
Adding SnCl2 to the cathode.
All of the above.
All of the above.
All of these changes would change Q and thus change the measured cell potential.
Example Question #671 : Ap Chemistry
For the following cell reaction:
2 Al (s) + 3 Mn2+ (aq) -> 2 Al3+ (aq) + 3 Mn (s)
predict if the cell potential Ecell will be larger, or smaller than Eocell for the following conditions:
[Al3+] = 2.0 M; [Mn2+] = 1.0 M.
Can not be determined
Identical
Smaller
Larger
Smaller
Altering these conditions would increase Q, and thus result in a decrease in the measured cell potential.
Example Question #71 : Thermodynamics
For the following cell reaction:
2 Al (s) + 3 Mn2+ (aq) -> 2 Al3+ (aq) + 3 Mn (s)
predict if the cell potential Ecell will be larger, or smaller than Eocell for the following conditions: [Al3+] = 1.0 M; [Mn2+] = 5.0 M.
Larger
Smaller
Identical
Can not be determined
Larger
At these concentrations Q will become smaller, and thus log Q will become smaller. This will give rise to a larger cell potential.
Example Question #72 : Thermodynamics
What is the cell potential of the following cell:
Zn (s) + 2 H+(aq) -> Zn2+ (aq) + H2 (g) Eo = 0.76 V
When the [Zn2+] = 1.0 M; PH2 = 1 atm, and the pH in the cathode is 5.2?
1.32 V
0.90 V
0.45 V
1.59 V
1.80 V
0.45 V
Example Question #682 : Ap Chemistry
Calculate the standard cell potential of the following reaction:
Cd(s) + MnO2 (s) + 4 H+ (aq) + -> Cd2+ (aq) + Mn2+ (aq) + 2 H2O (l)
Given:
MnO2 (s) + 4 H+ (aq) + 2e- -> Mn2+ (aq) + 2 H2O (l) Eo = 1.23 V
Cd2+ (aq) + 2 e- -> Cd (s) Eo = -0.40 V
0.0 V
-1.63 V
1.63 V
-0.83 V
0.83 V
1.63 V
Eocell = Eo cathode - Eoanode
Eocell = 1.23 – (-0.40) = 1.63 V
Example Question #1 : Cell Potential Under Non Standard Conditions
Calculate the standard cell potential of the following reaction:
Zn (s) + Cu2+ (aq) -> Zn2+ (aq) + Cu (s)
Given:
Zn2+(aq)+ 2 e--> Zn (s) Eo = -0.76 V
Cu2+(aq)+ 2 e--> Cu (s) Eo = 0.34 V
0.0 V
0.42 V
-0.42 V
-1.10 V
1.10 V
1.10 V
Eocell = Eo cathode - Eoanode
Eocell = 0.34 – (-0.76) = 1.10 V
Example Question #4 : Cell Potential Under Non Standard Conditions
Calculate the standard cell potential of the following reaction:
Zn (s) + 2 Ag1+ (aq) -> Zn2+ (aq) + 2 Ag (s)
Given:
Zn2+(aq)+ 2 e--> Zn (s) Eo = -0.76 V
Ag1+(aq)+ 1 e--> Ag (s) Eo = 0.80 V
-1.56 V
1.56 V
0.04 V
2.36 V
-0.04 V
1.56 V
Eocell = Eo cathode - Eoanode
Eocell = 0.80 – (-0.76) = 1.56 V
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