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Standard XII

Chemistry

SHE

Which cell of...

Question

Which cell of the following will measure standard electrode potential of copper electrode?

P t_{(s)} | H_{2} (g, 0.1 b a r) | H^{+} (a q, 1 M) | | C u^{2 +} (a q, 1 M) | C u

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P t_{(s)} | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | C u^{2 +} (a q, 2 M) | C u

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P t_{(s)} | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | C u^{2 +} (a q, 1 M) | C u

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P t_{(s)} | H_{2} (g, 1 b a r) | H^{+} (a q, 0.1 M) | | C u^{2 +} (a q, 1 M) | C u

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Solution

The correct option is C $P t_{(s)} | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | C u^{2 +} (a q, 1 M) | C u$
Standard hydrogen electrode as anode coupled with $C u$ as cathode measures the cell potential of $C u$ electrode.
$P t_{(s)} | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | C u^{2 +} (1 M) | C u$
Standard conditions.

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Similar questions

Q. If

E_{C u | C u^{+}}^{0} = - 0.53 V

and

E_{C u^{+} | C u^{2 +}}^{0} = - 0.15 V

For given cell,

P t (s) | H_{2} (g, 101325 p a s c a l) | H_{2} S O_{4} (a q .) | | C u^{2 +} (a q ., 1 M) | C u (s)

E_{c e l l} = 0.34 V a t 298 K

Then, the molarity of

H_{2} S O_{4} (a q .)

solution is equal to:

Q. For the following electrochemical cell at 298K,

P t (s) | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | M^{4 +} (a q), M^{2 +} (a q) | P t (s)

E_{c e l l} = 0.092

V when

\frac{[M^{2 +} (a q)]}{[M^{4 +} (a q)]} = 10^{x}

Given

: E_{M^{4 +} / M^{2 +}}^{0} = 0.151 V; 2.303 \frac{R T}{F} = 0.059 V

The value of x is :

Q. For the following electrochemical cell at 298 K,

P t (s) | H_{2} (g, 1 b a r) | H^{+} (a q, 1 M) | | M^{4 +} (a q), M^{2 +} (a q) | P t (s)

E_{c e l l} = 0.092 V w h e n \frac{[M^{2 +} + (a q)]}{[M^{4 +} (a q)]} = 10^{x}

G i v e n : E_{M^{4 +} / M^{2 +}}^{\circ} = 0.151 V; 2.303 \frac{R T}{F} = 0.059 V

The value of x is

In the electrochemical cell $P t (s) | H_{2} (g), 1 a t m | H^{+} (1 M) | | C u^{2 +} (1 M) | C u (s)$ , which one of the following statements is true?

Q. If

E_{C u | C u^{+}}^{0} = - 0.53 V

and

E_{C u^{+} | C u^{2 +}}^{0} = - 0.15 V

For given cell,

P t (s) | H_{2} (g, 101325 p a s c a l) | H_{2} S O_{4} (a q .) | | C u^{2 +} (a q ., 1 M) | C u (s)

E_{c e l l} = 0.34 V a t 298 K

Then, the molarity of

H_{2} S O_{4} (a q .)

solution is equal to:

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Which cell of the following will measure standard electrode potential of copper electrode?

The correct option is C Pt(s)|H2(g,1bar)|H+(aq,1M)||Cu2+(aq,1M)|CuStandard hydrogen electrode as anode coupled with Cu as cathode measures the cell potential of Cu electrode.Pt(s)|H2(g,1bar)|H+(aq,1M)||Cu2+(1M)|CuStandard conditions.