MHT CET 2025 26th April Morning Shift | Electrochemistry Question 1 | Chemistry

For the cell reaction, $\mathrm{A}_{(\mathrm{s})}+\mathrm{B}_{(\mathrm{eq})}^{+_2} \longrightarrow \mathrm{~A}_{(\mathrm{eq})}^{+_2}+\mathrm{B}_{(\mathrm{s})}$ if equilibrium constant of reaction is $10^4$ at 298 K . What is standard emf of cell?

0.0592 V

0.1184 V

0.1776 V

0.2368 V

MHT CET 2025 26th April Morning Shift

MCQ (Single Correct Answer)

-0

If $\mathrm{E}^{-}\left(\mathrm{Cu}_{(a q)}^{+2} \mid \mathrm{Cu}_{(s)}\right)=+0.34 \mathrm{~V}$. What is potential for $\mathrm{Cu}_{(s)} \rightarrow \mathrm{Cu}_{(\mathrm{aq})}^{+2}(0.1 \mathrm{M})+2 \mathrm{e}^{-}$at 298 K ?

+0.3696 V

-0.3696 V

+0.3104 V

-0.3104 V

MHT CET 2025 25th April Evening Shift

MCQ (Single Correct Answer)

-0

If standard reduction potential $\left(\mathrm{E}^{\circ}\right)$ of $\left(\mathrm{Mg}_{(\mathrm{aq})}^{+2} \mid \mathrm{Mg}_{(\mathrm{s})}\right),\left(\mathrm{Ag}_{(\mathrm{aq})}^{+} \mid \mathrm{Ag}_{(\mathrm{s})}\right),\left(\mathrm{Zn}^{+2}{ }_{(\mathrm{aq})} \mid \mathrm{Zn}_{(\mathrm{s})}\right)$ and $\left(\mathrm{Cu}^{+2}{ }_{(\text {aq })} \mid \mathrm{Cu}_{(\text {s })}\right)$ are $-2.37 \mathrm{~V},+0.79 \mathrm{~V},-0.76 \mathrm{~V}$ and +0.34 V respectively. Which of the following reaction is spontaneous?

$\quad \mathrm{Zn}_{(\mathrm{s})}+\mathrm{Mg}_{(\mathrm{aq})}^{+2} \longrightarrow \mathrm{Zn}_{(\mathrm{aq})}^{+2}+\mathrm{Mg}_{(\mathrm{s})}$

$\quad 2 \mathrm{Ag}_{(\mathrm{s})}+\mathrm{Zn}_{(\mathrm{aq})}^{+2} \longrightarrow 2 \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{Zn}_{(\mathrm{s})}$

$\mathrm{Zn}_{(\mathrm{s})}+\mathrm{Cu}_{(\mathrm{aq})}^{+2} \longrightarrow \mathrm{Zn}_{(\mathrm{aq})}^{+2}+\mathrm{Cu}_{(\mathrm{s})}$

$\quad \mathrm{Cu}_{(\mathrm{s})}+\mathrm{Mg}_{(\mathrm{aq})}^{+2} \longrightarrow \mathrm{Cu}_{(\mathrm{aq})}^{+2}+\mathrm{Mg}_{(\mathrm{s})}$

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