During the charging of a lead storage battery,the reaction at the anode is:

Give the chemical reaction when a $Cu$ rod is kept in an $AgNO_{3}$ solution.

An electrochemical cell is constructed using half-cells in the direction of spontaneous change: $Fe(OH)_{2}(s) + 2e^{-} \rightarrow Fe(s) + 2OH^{-}(aq)$ $(E^{0} = -0.88 \text{ V})$ and $AgBr(s) + e^{-} \rightarrow Ag(s) + Br^{-}(aq)$ $(E^{0} = +0.07 \text{ V})$. Which of the following options is correct?

$A$ variable,opposite external potential $(E_{ext})$ is applied to the cell $Zn | Zn^{2+} (1 \ M) || Cu^{2+} (1 \ M) | Cu$ of potential $1.1 \ V$. When $E_{ext} < 1.1 \ V$ and $E_{ext} > 1.1 \ V$,respectively,electrons flow from:

Given $\lambda^{\circ}_{Mg^{2+}} = 106 \ S \ cm^2 \ mole^{-1}$ and $\lambda^{\circ}_{SO_4^{2-}} = 160 \ S \ cm^2 \ mole^{-1}$. The value of $\lambda^{\circ}_{MgSO_4}$ (in $S \ cm^2 \ mole^{-1}$) is

What is the correct cell representation for the reaction $2Br^{-}_{(aq)} + Cl_{2(g)} \rightarrow Br_{2(l)} + 2Cl^{-}_{(aq)}$?