For the following chemical equation: Cu(s) + 2 H+ (aq) −−→ Cu2+(aq) + H2 (g) determine: 6a. The number of electrons exchanged per mole reaction 6b. Standard cell potential E ◦ given ∆G◦ rxn at 298 K 6c. What is the pH for which the cell potential E = 0 volts, when [Cu2+]−−1 M and pH2 = 1 atm at 298 K?
For the following chemical equation: Cu(s) + 2 H+ (aq) −−→ Cu2+(aq) + H2 (g) determine: 6a. The number of electrons exchanged per mole reaction 6b. Standard cell potential E ◦ given ∆G◦ rxn at 298 K 6c. What is the pH for which the cell potential E = 0 volts, when [Cu2+]−−1 M and pH2 = 1 atm at 298 K?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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For the following chemical equation: Cu(s) + 2 H+ (aq) −−→ Cu2+(aq) + H2 (g) determine:
6a. The number of electrons exchanged per mole reaction
6b. Standard cell potential E ◦ given ∆G◦ rxn at 298 K
6c. What is the pH for which the cell potential E = 0 volts, when [Cu2+]−−1 M and pH2 = 1 atm at 298 K?
![Useful info
NA = 6.022×1023 mọl!
g = 9.807 m/s?
1 bar = 10° Pa
1 atm = 1.013bar
= 760 Torr
1 mbar = 103 bar
R = 8.314 J/K-mol
= 8.206x10 L-atnm/K-mol
= 8.206x10° m²-atm/K-mol
= 62.36 L-Torr/K-mol
1J = 10² L-bar = 9.870×10³ L-atm = 0.2390 cal
1m=10° cm= 10° mm = 10° µm = 10° nm
1 -atm = 101.3 J
1 m³ = 10° L = 10° cm³
1 kg = 1000 g
1 Watt (W) = 1 J/s
1 Volt (V) = 1 J/Coulomb
1 Coulomb (C) = 6.24 x 1018 elementary charges
F = 9.645 x 104 C/mol
At 298 K (only):
RT = 2.478 kJ/mol (= 24.46 L-atm/mol)
RT/F = 0.0257 V (= 25.7 mV)
Pm[H>O] =1.00 g/mL
1010 A
Physical Properties of Selected Substances
mol. wt.
So
Cp,m
ΔΗ
melting temp AH
boiling temp
fus
m
vap
g/mol
32.04
kJ/mol
J/(mol-K) J/(mol-K) kJ/mol
126.8
239.8
K
kJ/mol
K.
CH;OH(1)
CH,OH(g)
C,H,(1)
C[(aq)
Cu(s)
-238.66
3.16
175.2
35.29
337.2
32.04
-200.66
78.1
+49.0
173.3
136.1
2.9
278.6
30.8
353.3
35.45
-167.16
56.5
-136.4
24.4
63.5
33.2
H2(g)
H*(aq)
H,O(1)
H,O(g)
Na*(aq)
NaCI(s)
2.0
131.7
28.8
1.01
18.0
-285.8
69.9
75.3
6.0
273
40.6
373
18.0
-241.8
188.8
33.6
23.0
-240.1
59.0
46.4
58.4
-411.5
72.1
50.5
Properties of pure phases are for standard conditions of 298 K and 1 atm.
Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm.
Integrals
+1
r"dr
;n + -1
%3D
n+1
Freezing and boiling point constants
Kf, K-kg/mol Kp, K-kg/mol
1.86
dr
Inz
Water
Benzene, C,H,
0.51
1
5.12
2.53
- In(az – b)
rp-
Nomenclature – but, when in doubt, write it out!
AG Change in Gibbs free energy for an arbitrary process (energy)
AGxn Molar Gibbs free energy change of reaction = (@G/a£)T,p (energy/mole)
AGn Standard Gibbs free change of reaction, per mole, between separated products and reactants, each in the
standard states for the phases specified. (energy/mole)
rxn](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F92fc06c1-ccdf-43d5-8f97-ed38225f057b%2Fbca413c5-66fd-48d8-b4f6-5d05d7c142bf%2Fv3cb771_processed.png&w=3840&q=75)
Transcribed Image Text:Useful info
NA = 6.022×1023 mọl!
g = 9.807 m/s?
1 bar = 10° Pa
1 atm = 1.013bar
= 760 Torr
1 mbar = 103 bar
R = 8.314 J/K-mol
= 8.206x10 L-atnm/K-mol
= 8.206x10° m²-atm/K-mol
= 62.36 L-Torr/K-mol
1J = 10² L-bar = 9.870×10³ L-atm = 0.2390 cal
1m=10° cm= 10° mm = 10° µm = 10° nm
1 -atm = 101.3 J
1 m³ = 10° L = 10° cm³
1 kg = 1000 g
1 Watt (W) = 1 J/s
1 Volt (V) = 1 J/Coulomb
1 Coulomb (C) = 6.24 x 1018 elementary charges
F = 9.645 x 104 C/mol
At 298 K (only):
RT = 2.478 kJ/mol (= 24.46 L-atm/mol)
RT/F = 0.0257 V (= 25.7 mV)
Pm[H>O] =1.00 g/mL
1010 A
Physical Properties of Selected Substances
mol. wt.
So
Cp,m
ΔΗ
melting temp AH
boiling temp
fus
m
vap
g/mol
32.04
kJ/mol
J/(mol-K) J/(mol-K) kJ/mol
126.8
239.8
K
kJ/mol
K.
CH;OH(1)
CH,OH(g)
C,H,(1)
C[(aq)
Cu(s)
-238.66
3.16
175.2
35.29
337.2
32.04
-200.66
78.1
+49.0
173.3
136.1
2.9
278.6
30.8
353.3
35.45
-167.16
56.5
-136.4
24.4
63.5
33.2
H2(g)
H*(aq)
H,O(1)
H,O(g)
Na*(aq)
NaCI(s)
2.0
131.7
28.8
1.01
18.0
-285.8
69.9
75.3
6.0
273
40.6
373
18.0
-241.8
188.8
33.6
23.0
-240.1
59.0
46.4
58.4
-411.5
72.1
50.5
Properties of pure phases are for standard conditions of 298 K and 1 atm.
Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm.
Integrals
+1
r"dr
;n + -1
%3D
n+1
Freezing and boiling point constants
Kf, K-kg/mol Kp, K-kg/mol
1.86
dr
Inz
Water
Benzene, C,H,
0.51
1
5.12
2.53
- In(az – b)
rp-
Nomenclature – but, when in doubt, write it out!
AG Change in Gibbs free energy for an arbitrary process (energy)
AGxn Molar Gibbs free energy change of reaction = (@G/a£)T,p (energy/mole)
AGn Standard Gibbs free change of reaction, per mole, between separated products and reactants, each in the
standard states for the phases specified. (energy/mole)
rxn
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