(A) During electrolysis,the ion with the higher standard reduction potential $(E^{\circ})$ is reduced first at the cathode.Comparing the given values:

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(A) During electrolysis,the ion with the higher standard reduction potential $(E^{\circ})$ is reduced first at the cathode.Comparing the given values:$E^{\circ}_{A^{2+}/A} = 0.8 \ V$$E^{\circ}_{B^{3+}/B} = 0.6 \ V$Since $0.8 \ V > 0.6 \ V$,the ion $A^{2+}_{(aq.)}$ has a higher reduction potential.Therefore,$A^{2+}_{(aq.)}$ will be deposited first at the cathode.

Class 12 Chemistry Electrochemistry Electrochemical cells

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$A^{2+}_{(aq.)} + 2e^- \to A_{(s)}$ ; $E^{\circ} = 0.8 \ V$
$B^{3+}_{(aq.)} + 3e^- \to B_{(s)}$ ; $E^{\circ} = 0.6 \ V$
Using the above information,find the ion which will be deposited first at the cathode if a solution containing $A^{2+}_{(aq.)}$ and $B^{3+}_{(aq.)}$ is electrolysed.

A
$A^{2+}_{(aq.)}$
B
$B^{3+}_{(aq.)}$
C
$H^{+}_{(aq.)}$
D
$OH^{-}_{(aq.)}$

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The electrochemical cell is set up as follows: $Pt (H_2, 1 \, atm) | HCl (0.1 \, M) || \text{Acetic Acid} (0.1 \, M) | (H_2, 1 \, atm) Pt$. The $E.M.F.$ of the cell is not zero because:

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Efficiency of a cell with cell reaction under standard conditions,$A_{(s)} + B^{+} \to A^{+} + B_{(s)}$; $\Delta H^o = -300 \ kJ$ is $70\%$. The standard electrode potential of the cell is :- .................... $V$

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An electrochemical cell is set up as follows: $Pt(H_2, 1 \, atm) | 0.1 \, M \, HCl || 0.1 \, M \, CH_3COOH | (H_2, 1 \, atm) Pt$. The $E.M.F.$ of this cell will not be zero because:

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Copper displaces which of the following metals from their salt solutions?

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The equilibrium constant for the reaction $Zn_{(s)} + Sn^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Sn_{(s)}$ is $1 \times 10^{20}$ at $298 \ K$. The magnitude of standard electrode potential of $Sn/Sn^{2+}$ if $E_{Zn^{2+}/Zn}^0 = -0.76 \ V$ is $............ \times 10^{-2} \ V$. (Nearest integer)
Given : $\frac{2.303 \ RT}{F} = 0.059 \ V$

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$A^{2+}_{(aq.)} + 2e^- \to A_{(s)}$ ; $E^{\circ} = 0.8 \ V$$B^{3+}_{(aq.)} + 3e^- \to B_{(s)}$ ; $E^{\circ} = 0.6 \ V$Using the above information,find the ion which will be deposited first at the cathode if a solution containing $A^{2+}_{(aq.)}$ and $B^{3+}_{(aq.)}$ is electrolysed.

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The electrochemical cell is set up as follows: $Pt (H_2, 1 \, atm) | HCl (0.1 \, M) || \text{Acetic Acid} (0.1 \, M) | (H_2, 1 \, atm) Pt$. The $E.M.F.$ of the cell is not zero because:

Efficiency of a cell with cell reaction under standard conditions,$A_{(s)} + B^{+} \to A^{+} + B_{(s)}$; $\Delta H^o = -300 \ kJ$ is $70\%$. The standard electrode potential of the cell is :- .................... $V$

An electrochemical cell is set up as follows: $Pt(H_2, 1 \, atm) | 0.1 \, M \, HCl || 0.1 \, M \, CH_3COOH | (H_2, 1 \, atm) Pt$. The $E.M.F.$ of this cell will not be zero because:

Copper displaces which of the following metals from their salt solutions?

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$A^{2+}_{(aq.)} + 2e^- \to A_{(s)}$ ; $E^{\circ} = 0.8 \ V$
$B^{3+}_{(aq.)} + 3e^- \to B_{(s)}$ ; $E^{\circ} = 0.6 \ V$
Using the above information,find the ion which will be deposited first at the cathode if a solution containing $A^{2+}_{(aq.)}$ and $B^{3+}_{(aq.)}$ is electrolysed.