For the cell Ag(s)| Ag+(aq) | | Cu2+(aq) | Cu(s) , the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f is

Question

For the cell Ag(s)| Ag+(aq) | | Cu2+(aq) | Cu(s) , the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f is (A)  -1.136 volt (B)  1.136 volt (C)  - 0.462 volt (D)  0.462 volt

Tardigrade Admin · Accepted Answer

E° textcell = E° text(right hand electrode)- Ag(s) | Ag+(aq)| | Cu2+ (aq)| Cu E° text(Left hand electrode) E° /V LHS RHS Electrode Ag+ +2e- leftharpoons Ag 0.337 Cu2+ + 2e- leftharpoons Cu 0.799 E° textcell = RHS - LHS = 0.799 - 0.337 = 0.462 Volt

Q. For the cell $A g_{(s)} ∣ A g_{(a q)}^{+} ∣∣ C u_{(a q)}^{2 +} ∣ C u_{(s)}$ , the reduction potentials of the left and right hand electrodes are $0.337$ and $0.799$ volts, the cell $e . m . f$ is

$- 1.136$ volt

$1.136$ volt

$- 0.462$ volt

$0.462$ volt

Q. For the cell Ag(s)​∣Ag(aq)+​∣∣Cu(aq)2+​∣Cu(s)​ , the reduction potentials of the left and right hand electrodes are 0.337 and 0.799 volts, the cell e.m.f is

−1.136 volt

1.136 volt

−0.462 volt

0.462 volt

Ecell∘​=E(right hand electrode)-∘​ Ag(s)∣Ag+(aq)∣∣Cu2+(aq)∣CuE(Left hand electrode)∘​ E∘/V LHSRHS Electrode Ag++2e−⇌Ag0.337 Cu2++2e−⇌Cu0.799 Ecell∘​=RHS−LHS =0.799−0.337=0.462 Volt

Q. For the cell $A g_{(s)} ∣ A g_{(a q)}^{+} ∣∣ C u_{(a q)}^{2 +} ∣ C u_{(s)}$ , the reduction potentials of the left and right hand electrodes are $0.337$ and $0.799$ volts, the cell $e . m . f$ is

$- 1.136$ volt

$1.136$ volt

$- 0.462$ volt

$0.462$ volt