(a) (i) Calculate E_cell^0 for the following reaction which is at equilibrium: Cu ( s )+2 Ag^+( aq ) ⇌ Cu^2+( aq )+2 Ag ( s ) Equilibrium constant (…

Calculate $\displaystyle \mathrm{E}_{\text {cell }}^{0}$ for the following reaction which is at equilibrium : $\displaystyle \mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightleftharpoons \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$ Equilibrium constant $\displaystyle \left(\mathrm{K}_{\mathrm{c}}\right)$ for the cell is $\displaystyle 10^{15}$. [Given : $\displaystyle \log 10=1$ ]

Write anode, cathode and overall reaction of lead storage battery when it is in use.

How much electricity is required in coulombs for the oxidation of $\displaystyle 1$ mol of FeO to $\displaystyle \mathrm{Fe}_{2} \mathrm{O}_{3}$ ?

Conductivity of $\displaystyle 0.0024$ M acetic acid is $\displaystyle 7 \cdot 2 \times 10^{-5} \mathrm{~S} \mathrm{~cm}^{-1}$. If $\displaystyle \mathbf{\Lambda}_{\mathrm{m}}^{\circ}$ for acetic acid is $\displaystyle 390 \cdot 5 \mathrm{~S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}$, then calculate the degree of dissociation ( $\displaystyle \alpha$ ) of acetic acid.

Calculate the cell potential for the following half cell reaction at $\displaystyle 25$°C : \[\mathrm{Ag}^{+}(\mathrm{aq})+1 \mathrm{e}^{-} \longrightarrow \mathrm{Ag}(\mathrm{~s}) \] Given that : $\displaystyle \left[\mathrm{Ag}^{+}\right]=0.01 \mathrm{M}$ and \[\mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathrm{o}}=+0.80 \mathrm{~V} \] $\displaystyle [\log 10=1]$

Write the name of the electrolyte used in :

Dry cell

Fuel cell $\displaystyle \left(\mathrm{H}_{2}-\mathrm{O}_{2}\right)$