(A) The standard reduction potential $(\text{SRP})$ for $Cu^{2+} + 2e^{-} \rightarrow Cu$ is $+0.34 \ V$.The $\text{SRP}$ for $2H^{+} + 2e^{-} \righta

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(A) The standard reduction potential $(\text{SRP})$ for $Cu^{2+} + 2e^{-} \rightarrow Cu$ is $+0.34 \ V$.The $\text{SRP}$ for $2H^{+} + 2e^{-} \rightarrow H_2$ is $0.00 \ V$.Since the $\text{SRP}$ of $Cu^{2+}$ $(+0.34 \ V)$ is greater than the $\text{SRP}$ of $H^{+}$ $(0.00 \ V)$,$Cu^{2+}$ ions are reduced more easily than $H^{+}$ ions.Therefore,both the Assertion and the Reason are true,and the Reason correctly explains the Assertion.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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Assertion : $Cu^{2+}$ ions get reduced more easily than $H^{+}$ ions.
Reason : Standard electrode potential of copper is $0.34 \ V$.

A
Both Assertion and Reason are true
B
Both Assertion and Reason are false.
C
Assertion is true but Reason is false.
D
Assertion is false but Reason is true.

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Electrochemistry

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Electrode potential and ECell

The standard reduction potential values of the three metallic cations $x, y, z$ are $0.52 \ V, -3.03 \ V$ and $-1.18 \ V$ respectively. The order of reducing power of their corresponding metals will be

Medium

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If in a galvanic cell,the hydrogen half-cell is the cathode on the right side,what is the sign of the standard electrode potential of such a galvanic cell? Give an example.

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Given the standard electrode potentials: $Fe^{2+}_{(aq)} + 2e^{-} \rightarrow Fe_{(s)}$ $(E^o = -0.44 \ V)$ and $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ $(E^o = 0.77 \ V)$. If $Fe^{2+}$,$Fe^{3+}$,and a piece of $Fe$ are kept together,what happens?

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Given at $298 \ K$: $E^\ominus_{Fe^{2+}/Fe} = X \ V$; $E^\ominus_{Fe^{3+}/Fe} = Y \ V$. The $E^\ominus_{Fe^{3+}/Fe^{2+}}$ in Volt at $298 \ K$ is given by:

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Fill in the blanks :
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......

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Assertion : $Cu^{2+}$ ions get reduced more easily than $H^{+}$ ions.Reason : Standard electrode potential of copper is $0.34 \ V$.

Similar Questions

The standard reduction potential values of the three metallic cations $x, y, z$ are $0.52 \ V, -3.03 \ V$ and $-1.18 \ V$ respectively. The order of reducing power of their corresponding metals will be

If in a galvanic cell,the hydrogen half-cell is the cathode on the right side,what is the sign of the standard electrode potential of such a galvanic cell? Give an example.

Given the standard electrode potentials: $Fe^{2+}_{(aq)} + 2e^{-} \rightarrow Fe_{(s)}$ $(E^o = -0.44 \ V)$ and $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ $(E^o = 0.77 \ V)$. If $Fe^{2+}$,$Fe^{3+}$,and a piece of $Fe$ are kept together,what happens?

Given at $298 \ K$: $E^\ominus_{Fe^{2+}/Fe} = X \ V$; $E^\ominus_{Fe^{3+}/Fe} = Y \ V$. The $E^\ominus_{Fe^{3+}/Fe^{2+}}$ in Volt at $298 \ K$ is given by:

Fill in the blanks :$1$. ...... metal is the strongest reducing agent in aqueous solution.$2$. ...... gas is the strongest oxidizing agent.$3$. The standard reduction potential of any electrode is measured with reference to ......

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Assertion : $Cu^{2+}$ ions get reduced more easily than $H^{+}$ ions.
Reason : Standard electrode potential of copper is $0.34 \ V$.

Fill in the blanks :
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......