For a certain redox reaction in galvanic cell $\text{X}_{(s)} + \text{Y}^{2+}_{(aq)} \longrightarrow \text{X}^{2+}_{(aq)} + \text{Y}_{(s)}$, $\text{E}^\circ$ cell is $0.0296\ \text{V}$ at $298\ \text{K}$. What is equilibrium constant of reaction?

Which of the following net cell reactions occurs in a galvanic cell containing cadmium electrode and standard hydrogen electrode?
$\text{E}^\circ_{(\text{Cd}^{2+}_{(aq)}|\text{Cd}_{(s)})} = -0.403\ \text{V}$.

In a first order reaction 20 millimole of reactant is lowered to 10 millimole in $0.3010$ minute. Find rate constant of the reaction?

For the reaction $2\text{NOBr}_{(g)} \longrightarrow 2\text{NO}_{(g)} + \text{Br}_{2(g)}$, rate law is $r = k[\text{NOBr}]^2$. Rate constant is $1.62\ \text{M s}^{-1}$ and concentration of NOBr is $5 \times 10^{-3}\ \text{M}$,
What is rate of reaction?