Use tabulated half-cell potentials to calculate ΔG∘rxn for each
of the following reactions at 25 ∘C.
Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)
Express the energy change in kilojoules to two significant
figures.
Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq)
Express the energy change in kilojoules to one significant
figure.
Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express
the energy change in kilojoules to two significant figures.
For each of the following reactions, calculate ?H?rxn,
?S?rxn, ?G?rxn at 25?C. State whether or not the
reaction is spontaneous. If the reaction is not spontaneous, would
a change in temperature make it spontaneous? If so, should the
temperature be raised or lowered from 25?C?
2CH4(g)?C2H6(g)+H2(g)
?H?rxn, ?S?rxn, ?G?rxn at 25?C???
Use the tabulated half-cell potentials below to calculate the
equilibrium constant (K) for the following balanced redox reaction
at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)
For each of the following reactions, calculate ΔH∘rxn,
ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not
the reaction is spontaneous. If the reaction is not spontaneous,
would a change in temperature make it spontaneous? If so, should
the temperature be raised or lowered from 25
∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C.
2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C.
N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C.
2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.
For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn,
ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous.
If the reaction is not spontaneous, would a change in temperature
make it spontaneous? If so, should the temperature be raised or
lowered from 25 ∘C?
a) 2CH4(g)→C2H6(g)+H2(g)
b) 2NH3(g)→N2H4(g)+H2(g)
c) N2(g)+O2(g)→2NO(g)
d) 2KClO3(s)→2KCl(s)+3O2(g)
Can you please show equations. I am having so much trouble with
these.
1)For each of the following reactions, calculate
ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C.
3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g)
N2(g)+3H2(g)→2NH3(g)
2)Before investigating the scene, the technician must dilute the
luminol solution to a concentration of
6.00×10−2M . The diluted solution is then
placed in a spray bottle for application on the desired
surfaces.
How many moles of luminol are present in 2.00 L of the diluted
spray?
3)A student placed 11.0 g of glucose (C6H12O6) in a volumetric
flask, added enough water to dissolve...
Calculate the equilibrium constant for each of the reactions at
25∘C.
Standard Electrode Potentials at 25 ∘C
Reduction Half-Reaction
E∘(V)
Fe3+(aq)+3e−
→Fe(s)
-0.036
Sn2+(aq)+2e−
→Sn(s)
-0.14
Ni2+(aq)+2e−
→Ni(s)
-0.23
O2(g)+2H2O(l)+4e−
→4OH−(aq)
0.40
Br2(l)+2e−
→2Br−
1.09
I2(s)+2e−
→2I−
0.54
Part A
2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)
Express your answer using two significant figures.
Part B
O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq)
Express your answer using two significant figures.
Part C
Br2(l)+2I−(aq)→2Br−(aq)+I2(s)
Express your answer using two significant figures.
Use the following half-reactions to write three spontaneous
reactions, and calculate E cell for each reaction:
a. Au+ (aq) + e- ----> Au (s) E= 1.69
V
b. N2O (g) + 2H+ (aq) + 2 e-
----> N2 (g) + H2O (l) E= 1.77 V
c. Cr3+ (aq) + 3e- ---> Cr (s) E= -0.74
V
Calculate ?G?rxn and K for each of the
following reactions.
Part A
The reaction of Cr2+(aq) with
Cr2O2?7(aq) in acid solution to form
Cr3+(aq).
Calculate ?G?rxn.
Part B
Calculate K.
Express your answer using two significant figures.
Part C
The reaction of Cr3+(aq) and Cr(s) to form
Cr2+(aq). [The reduction potential of
Cr2+(aq) to Cr(s) is -0.91 V.]
Calculate ?G?rxn.
Express your answer using two significant figures.
Part D
Calculate K.
Express your answer using one significant figure.