List of top Chemistry Questions on Nernst Equation asked in KEAM

For $Zn(s)+Cu^{2+}(0.1M) \rightarrow Zn^{2+}(0.001 M)+Cu(s)$, calculate $E_{cell}$ if $E^0_{cell} = 1.1V$. ________.

Given the reaction: \[ \text{Cu(s)} + 2\text{Ag}^+_{(aq)} \rightleftharpoons \text{Cu}^{2+}_{(aq)} + 2\text{Ag(s)} \quad (\text{E}_{\text{cell}}^\circ = 0.295 \, \text{V}, \, 2.303 \, \frac{RT}{F} = 0.059 \, \text{V}) \] What is the value of the equilibrium constant \( K \)?

The electrode potential E$_{\left(\frac{Zn^{2+}}{Zn}\right)}$ of a zinc electrode at 25$^{\circ}$C with an aqueous solution of 0.1M $ZnSO_4$ is (E$^{\circ}$$_{\left(\frac{Zn^{2+}}{Zn}\right)}$ = -0.76 V. Assume $\frac{2.303RT}{F} =$ 0.06 at 298 K)

The standard electrode potentials of $ A{{g}^{+}}/Ag $ is $ +0.80\text{ }V $ and $ C{{u}^{+}}/Cu $ is $ +0.34\text{ }V $ . These electrodes are connected through a salt bridge and if: