What happens to the voltage if the salt bridge is suddenly removed from a working electrochemical cell?

Consider the Galvanic cell $Zn|ZnSO_4||CuSO_4|Cu$. The reaction at the cathode is

On charging the lead storage battery,the oxidation state of lead changes from $x_1$ to $y_1$ at the anode and from $x_2$ to $y_2$ at the cathode. The values of $x_1, y_1, x_2, y_2$ are respectively $:$

For the reaction $2 Fe^{3+}_{(aq)} + 2 I^{-}_{(aq)} \rightarrow 2 Fe^{2+}_{(aq)} + I_{2(s)}$,the magnitude of the standard molar free energy change,$\Delta_{r} G_{m}^{\circ} = -$ ........... $kJ$ (Round off to the Nearest Integer). $\left[ E_{Fe^{2+} / Fe_{(s)}}^{\circ} = -0.440 \ V; \ E_{Fe^{3+} / Fe_{(s)}}^{\circ} = -0.036 \ V; \ E_{I_{2} / 2I^{-}}^{\circ} = 0.539 \ V; \ F = 96500 \ C \ mol^{-1} \right]$

The energy conversion involved in a galvanic cell is

The charge over the anode in a galvanic cell is