Electrochemistr...

The half-cell reaction is the one that:

On passing one faraday of electricity through a dilute solution of an acid, the volume of hydrogen obtained at NTP is__________.

The half-cell reaction for the corrosion,
$$2H^{+} + \dfrac {1}{2}O_{2} + 2e^{-} \rightarrow H_{2}O; E^{\circ} = 1.23\ V$$
$$Fe^{2+} + 2e^{-} \rightarrow Fe(s); E^{\circ} = -0.44\ V$$
Find the $$\triangle G^{\circ}$$ (in kJ) for the overall reaction.

What is the sign of $$\triangle G^{\circ}$$ and the value of $$K$$ for a electrochemical cell for which $$E^{\circ}_{cell} = 0.80\ V$$?

The number of electrons involved when one faraday of electricity is passed through an electrolytic solution is:

For the cell reaction,
$$\underset {(C_{1})}{Cu^{2+}}(aq.) + Zn(s) \rightarrow \underset {(C_{2})}{Zn^{2+}}(aq.) + Cu(s)$$
the change in free energy $$(\triangle G)$$ at a given temperature is a function of____________.

The standard emf of a galvanic cell involving cell reaction with $$n = 2$$ is found to be $$0.295\ V$$ at $$25^{\circ}C$$. The equilibrium constant of the reaction would be:
Given: $$F = 96500\ C\ mol^{-1}; R = 8.314\ JK^{-1} mol^{-1}$$.

The measured potential for,
$$Mg^{2+} + 2e^{-}\rightleftharpoons Mg(s)$$
does not depend upon:

The main factors which affect corrosion are :

Match the thermodynamic properties (List I) with their relation (List II).