8.Using the following standard reduction potentials: Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions. Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Pb(s) 9. Consider the reaction: N2(g) + 3 F2(g) → 2 NF3(g) ΔH° = -249 kJ and ΔS° = -278 J/K at 25°C Calculate ΔG° and state whether the equilibrium composition should favor reactants or products at standard conditions. 10. Calculate the standard free energy for the reaction given. 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) Species ΔGof (kJ/mol) CH3OH (l) -166.4 O2 (g) 0.0 CO2 (g) -394.4 H2O (l) -237.3
8.Using the following standard reduction potentials:
|
Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V |
|
Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V |
calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions.
Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Pb(s)
9.
Consider the reaction:
N2(g) + 3 F2(g) → 2 NF3(g) ΔH° = -249 kJ and ΔS° = -278 J/K at 25°C
Calculate ΔG° and state whether the equilibrium composition should favor reactants or products at standard conditions.
10.
Calculate the standard free energy for the reaction given.
2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l)
|
Species |
ΔGof (kJ/mol) |
|
CH3OH (l) |
-166.4 |
|
O2 (g) |
0.0 |
|
CO2 (g) |
-394.4 |
|
H2O (l) |
-237.3 |
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