(a) Calculate the standard Gibbs energy (\(\Delta G^\circ\)) of the following reaction at 25°C:
\(\text{Au(s) + Ca\(^{2+}\)(1M) $\rightarrow$ Au\(^{3+}\)(1M) + Ca(s)} \)
\(\text{E\(^\circ_{\text{Au}^{3+}/\text{Au}} = +1.5 V, E\)\(^\circ_{\text{Ca}^{2+}/\text{Ca}} = -2.87 V\)}\)
\(\text{1 F} = 96500 C mol^{-1}\)
Define the following:
(i) Cell potential
(ii) Fuel Cell
Calculate the emf of the following cell at 25°C:
\[ \text{Zn(s)} | \text{Zn}^{2+}(0.1M) || \text{Cd}^{2+}(0.01M) | \text{Cd(s)} \] Given: \[ E^\circ_{\text{Cd}^{2+}/\text{Cd}} = -0.40 \, V, \, E^\circ_{\text{Zn}^{2+}/\text{Zn}} = -0.76 \, V \] \[ [\log 10 = 1] \]
Write chemical equations of the following reactions:
(i) Phenol is treated with conc. HNO\(_3\)
(ii) Propene is treated with B\(_2\)H\(_6\) followed by oxidation by H\(_2\)O\(_2\)/OH\(^-\)
(iii) Sodium t-butoxide is treated with CH\(_3\)Cl
Give a simple chemical test to distinguish between butan-1-ol and butan-2-ol.