(A) The Nernst equation for the reduction half-reaction $M^+ + e^- \rightarrow M$ is given by:$E_{RP} = E^o_{RP} - \frac{0.059}{n} \log \frac{1}{[M^+]

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(A) The Nernst equation for the reduction half-reaction $M^+ + e^- \rightarrow M$ is given by:$E_{RP} = E^o_{RP} - \frac{0.059}{n} \log \frac{1}{[M^+]}$Given $E^o_{RP} = -2.36 \, V$,$[M^+] = 0.1 \, M$,and $n = 1$:$E_{RP} = -2.36 - 0.059 \log \frac{1}{0.1}$$E_{RP} = -2.36 - 0.059 \log(10)$Since $\log(10) = 1$:$E_{RP} = -2.36 - 0.059 = -2.419 \, V$

Class 12 Chemistry Electrochemistry Nernst equation and ECS

Medium

What is the reduction electrode potential $E$ of a $0.1 \, M$ solution of $M^{+}$ ions,given that the standard reduction potential $E^o_{RP} = -2.36 \, V$?

A
$-2.419 \, V$
B
$+0.241 \, V$
C
$-4.82 \, V$
D
None of these

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What is the reduction electrode potential $E$ of a $0.1 \, M$ solution of $M^{+}$ ions,given that the standard reduction potential $E^o_{RP} = -2.36 \, V$?

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For the reaction $A_{(s)} + 2B^{+}_{(aq)} \rightarrow A^{2+}_{(aq)} + 2B_{(s)}$,the value of $K_c$ is $10^{12}$. What is the value of $E^o_{cell}$ (in $, V$)?

In which of the following conditions will the reduction potential of a hydrogen half-cell be negative?

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