List of top Chemistry Questions on Electrochemical Cells asked in KEAM

Which of the following half-cell reaction has the most negative standard electrode potential?

What is the emf of the cell at $298\,K$ in which the following reaction takes place? \[ Ni(s) + 2Ag^+(0.002M) \rightarrow Ni^{2+}(0.04M) + 2Ag(s) \] ($E^\circ_{cell} = 1.05V$)

In the reaction, \( \text{O}_{2(g)} + 4\text{H}^+_{(aq)} + 4\text{e}^- \rightarrow 2\text{H}_2\text{O}_{(l)} \), the quantity of electricity required to reduce one mole of gaseous oxygen is ( \( E^\circ = 1.23\,\text{V} \) )

Which metal added in fuel cell to make it more efficient?

For which of the following electrode reactions the standard electrode potential is the highest at 298 K? The ions are present in aqueous solution. ________.

Which of the following statement is true for the electrochemical, Daniel cell?

The EMF of the cell at $298\ \text{K}$ is $Mg_{(s)}|Mg^{2+}(aq,\ 0.10\ \text{M})||Ag^{+}(aq,\ 0.001\ \text{M})|Ag_{(s)}$. (Given: $E^{0}_{cell}=3.17\ \text{V}$ and $\frac{2.303RT}{F}=0.06\ \text{V}$)

In Kolbe's electrolytic method, when sodium acetate is electrolysed, the gases generated at anode are

What is the quantity of current required to deposit one mole of metallic magnesium from fused magnesium chloride? (1F = 96500 C)

\( E_{\text{cell}} \) of the following cell is
\( \text{Pt(s)} \mid \text{H}_2\text{(g), 1 bar} \mid \text{H}^+ \text{ (1 M)} \mid\mid \text{H}^+ \text{ (0.1 M)} \mid \text{H}_2\text{(g), 1 bar} \mid \text{Pt(s)} \)

A fuel cell operates at constant current, with H$_2$ fuel (1 bar) and O$_2$ oxidant (1 bar). The electrolyte used is 0.001 M HCl and the product(s) of the reaction are confined inside the fuel cell. Which of the following is true about the electrolyte?

Consider a fuel cell supplied with 1 mole of H$_2$ gas and 10 moles of O$_2$ gas. If the fuel cell is operated at 96.5 mA current, how long will it deliver power? (Assume $1\ F = 96500\ \text{C/mol of electrons}$)

One gram of copper is deposited in a copper voltameter when a current of $0.5$ A flows for $30$ minutes. Then the current required to deposit $2$ g of silver in the same time is (ece of copper $= 3.3 \times 10^{-4}$ g C$^{-1}$, ece of silver $= 1.1 \times 10^{-3}$ g C$^{-1}$)

The standard electrode potentials of Zn and Ni are respectively $-0.76$ V and $-0.25$ V. Then the standard emf of the spontaneous cell by coupling these under standard conditions is

The change in potential of the half-cell Cu\textsuperscript{2+|Cu, when aqueous Cu\textsuperscript{2+} solution is diluted 100 times at 298 K? \(\left( \frac{2.303 RT}{F} = 0.06 \right)\)}

The change in potential of the half-cell Cu\textsuperscript{2+|Cu, when aqueous Cu\textsuperscript{2+} solution is diluted 100 times at 298 K? \(\left( \frac{2.303 RT}{F} = 0.06 \right)\)}

The change in potential of the half-cell Cu\textsuperscript{2+|Cu, when aqueous Cu\textsuperscript{2+} solution is diluted 100 times at 298 K? \(\left( \frac{2.303 RT}{F} = 0.06 \right)\)}