JEE CHEMISTRY MCQ: ELECTRO CHEMISTRY

1 Medium

1 of 1

Application +4 | -1

Iron powder is added to

1.0 \mathrm{~M}

solution of

{CdCl}_2

298 \mathrm{~K}

. The reaction occurring is

{Cd}^{2+}(a q)+{Fe}(s) \rightarrow {Cd}(s)+{Fe}^{2+}(a q)

. If the standard potential of a cell producing this reaction is

0.037 \mathrm{~V}

, the concentrations of

{Cd}^{2+}

and

{Fe}^{2+}

ions in the above reaction at equilibrium respectively will be (Hint:-

\left.10^{1.3}=20\right)

View answer and explanation

Correct option: A

0.05 \mathrm{~M}, 0.95 \mathrm{~M}

Option A (0.05 M, 0.95 M) is correct because it is calculated using the Nernst equation at equilibrium and the given standard potential.

More Questions from ELECTRO CHEMISTRY

Practice All Chapter MCQs →

25^{\circ} \mathrm{C}

0.295 \mathrm{~V}

{p_1}{\kern 1pt} {\kern 1pt} \mathrm{and}{\kern 1pt} {\kern 1pt} {p_2}

\mathop {\mathrm{Pt}\left( {{\mathrm{H}_2}} \right)}\limits_{{p_1}} \left| {\mathop {{\mathrm{H}^ + }\left( {aq} \right)}\limits_{1\mathrm{ }M} } \right|\mathop {Pt\left( {{\mathrm{H}_2}} \right)}\limits_{{p_2}}

\mathrm{CuS}{\mathrm{O}_4}

{AlCl}_3

STP

({F}=96500 {C})

2 \mathrm{Ag}(\mathrm{s})+\mathrm{S}^{2-}(\mathrm{aq}) \rightarrow \mathrm{Ag}_2 \mathrm{S}(\mathrm{s})+2 \mathrm{e}^{-}

\mathrm{pH}=3

0.1 \mathrm{~M}-\mathrm{H}_2 \mathrm{S},

\mathrm{H}_2 \mathrm{S}, K_{\mathrm{a}_1}=10^{-8} ; K_{\mathrm{a}_2}=10^{-13}, K_{\mathrm{sp}}

\mathrm{Ag}_2 \mathrm{S}=4 \times 10^{-48},

E^{\circ}_{{\mathrm{Ag} | \mathrm{Ag}}^{+}}=0.80 \mathrm{~V},

\log 2=0.3,

2.303 R T / F=0.06