List of top Chemistry Questions on Electrochemical Cells asked in COMEDK UGET

For a cell \( 2M(s) + O_2(g) + 4H^+ \rightarrow 2M^{2+}(aq) + 2H_2O(l) \), the \( E^\circ_{\text{cell}} = +1.67\,V \). When \( [M^{2+}] = 1.0 \times 10^{-3} \, M \) and \( p(O_2) = 0.1 \, atm \), the EMF of the cell becomes \( +1.57 \, V \). Calculate the pH of the electrochemical cell.

Identify the two incorrect electrochemical reactions shown as taking place in the given cells at the respective electrodes.

For the cell reaction \( 4Br^- + O_2 + 4H^+ \rightarrow 2Br_2 + 2H_2O \) at \( 298\,K \), the \( E^0_{\text{cell}} = 0.16\,V \). What would be the \( K_c \) (Equilibrium constant) value if the reverse reaction were to take place?

What is the standard electrode potential at 298 K for the reaction:
\[ \text{Cu}^{2+} + \text{e}^- \rightarrow \text{Cu}^+ \] Given: \( E^0_{\text{Cu}^{+}/\text{Cu}} = 0.5 \, \text{V} \) and \( E^0_{\text{Cu}^{2+}/\text{Cu}} = 0.335 \, \text{V} \)