What will be the $emf$ for the given cell $Pt|H_2(P_1)|H^{+}_{(aq)}||H_2(P_2)|Pt$?

The reduction potential of a hydrogen half-cell will be negative if:

For the reaction; $2A_{(s)} + B_{(aq)}^{2+} \to 2A_{(aq)}^{+} + B_{(s)}$,the Nernst equation for the $EMF$ of the cell is:

If $Zn/Zn^{+2}$ electrode is diluted $100$ times,then the change in electromotive force will be:

If $A$ is the reactant and $P$ is the product,which one of the following is the correct form of the Nernst equation?

An electrochemical cell consists of the following two redox couples, $M^{x+}(aq)/M(s)$ $[E^{\ominus}_{red} = +0.15 \text{ V}]$ and $Fe^{3+}(aq)/Fe(s)$ $[E^{\ominus}_{red} = -0.036 \text{ V}]$. The cell $EMF$ is recorded to be $0.2057 \text{ V}$. If the reaction quotient of the electrochemical reaction is found to be $10^{-2}$, then the value of $x$ is . . . . . . . (Nearest integer) [Given: $M$ is a $p$-block metal and $\frac{2.303RT}{F} = 0.059 \text{ V}$]