JEE CHEMISTRY MCQ: ELECTRO CHEMISTRY

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Application +4 | -1

Using the SRP values given below, decide which of the statements I, II, III and IV are correct.

\begin{array}{l} F{e^{2 + }} + 2{e^ - }\underset{{}}{\overset{{}}{\leftrightharpoons}}Fe\,;\,{E^\mathrm{o}} = - 0.44\,V\\ C{u^{ + 2}} + 2{e^ - }\underset{{}}{\overset{{}}{\leftrightharpoons}}Cu\,;\,{E^\mathrm{o}} = + 0.34\,V\\ A{g^ + } + {e^ - }\underset{{}}{\overset{{}}{\leftrightharpoons}}Ag\,;\,{E^\mathrm{o}} = + 0.80\,V \end{array}

(I) Copper can displace iron from

FeS{O_4}

solution
(II) Iron can displace copper from

CuS{O_4}

solution
(III) Silver can displace copper from

CuS{O_4}

solution
(IV) Iron can displace silver from

AgN{O_3}

solution

View answer and explanation

Correct option: C

II and IV

Option C (II and IV) is correct because iron can displace copper from copper sulfate solution and iron can displace silver from silver nitrate solution due to their relative SRP values.

More Questions from ELECTRO CHEMISTRY

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25^{\circ} \mathrm{C}

, the standard emf of cell having reactions involving two electron change is found to be

0.295 \mathrm{~V}

. The equilibrium constant of the reaction is Which are used as secondary reference electrodes? For the following cell with hydrogen electrodes at two different pressures

{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}}

emf is given by A current of strength 2.5 A was passed through

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

solution for 6 min 26 s. The amount of copper deposited is (At. Wt. of Cu = 63.5, 1F = 96500 C) A current strength of 9.65 amperes is passed through excess fused

{AlCl}_3

for 5 hours. How many litres of chlorine will be liberated at

STP

({F}=96500 {C})

The electrode potential (in millivolts) of

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

in a solution buffered at

\mathrm{pH}=3

and which is also saturated with

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

is (Given: for

\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

)