The electrode potential for Mg electrode varies according to the equation

$$E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}$$

The graph of EMg2+ / Mg vs log [Mg2+] among the following is:

 1 2 3 4
Subtopic:  Nernst Equation |
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${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}$= 1.1 V for Daniel cell. Which of the following expressions are correct descriptions of the state of equilibrium in this cell?

(a) 1.1 = KC

(b) $\frac{2.303\mathrm{RT}}{2\mathrm{F}}{\mathrm{logK}}_{\mathrm{C}}=1.1$

(c) ${\mathrm{logK}}_{\mathrm{C}}=\frac{2.2}{0.059}$

(d) log KC = 1.1

The correct choice among the given is -

1. (a, b)

2. (b, c)

3. (c, d)

4. (a, d)

Subtopic:  Nernst Equation |
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For the given cell, Mg | Mg2+ || Cu2+ | Cu

a.  Mg acts as cathode

b.  Cu acts as cathode

c.  The cell reaction is   $$Mg + Cu^{2+} \rightarrow Mg^{2+} + Cu$$

d.  Cu is the oxidising agent

The correct choice among the given is -

1. (a, b)
2. (b, c)
3. (c, d)
4. (a, d)

Subtopic:  Electrolytic & Electrochemical Cell | Nernst Equation |
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