Nonstandard Concentrations and Cell Potential The value of E^degree for the foll

Question

Nonstandard Concentrations and Cell Potential

The value of E^degree for the following reaction is 1.10 V. What is the value of E_cell when the concentration of Cu^2+ is 1.0 M and the concentration of Zn^2+ is 0.025 M? Zn(s) + Cu^2+(aq) rightarrow Cu(s) + Zn^2+(aq) E^degree = 1.10 V a. 1.40 V b. 0.95 V c. 1.15 V d. 0.80 V The value of E^degree for the following reaction is 1.260 V. What is the value of E_cell given the concentrations shown? 2Al(s) + 3Cd^2+(aq) rightarrow 3Cd(s) + 2Al^3+(aq) 0.1 M 0.6 M E^degree = 1.260 V a. 1.235 V b. 1.285 V c. 1.15 V d. 1.37 V The value of E^degree for the following reaction is 0.189 V. What is the value of E_cell given the concentrations shown? 4H^+(aq) + Fe(s) + NO_3^-(aq) rightarrow Fe^3+(aq) + NO(aq) + 2H_2O(l) E^degree = 0.189 V 0.1 M 0.6 M 1.0 M 0.5 M a. -0.215 V b. 0.112 V c. 0.189 V d. 0.266 V

Explanation / Answer

59)
the number of electron being transferred, n = 2

use:
E = Eo - (0.0592/n) * log {[Zn2+]/[Cu2+]}
= 1.10 - (0.0592/2)* log (0.025/1.0)
= 1.10 + 0.05
= 1.15 V

Answer: c

60)
the number of electron being transferred, n = 6

use:
E = Eo - (0.0592/n) * log {[Al3+]^2/[Cd2+]^3}
= 1.260 - (0.0592/6)* log (0.6^2/0.1^3)
= 1.260 - (0.0592/6)*log (360)
= 1.260 - 0.025
= 1.235 V
Answer: a

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