Question

The overall reaction in the lead storage battery is

Answer 1

Complete Question

The overall reaction in the lead storage battery is

$Pb(s) + PbO2(s) + 2H(aq)^+ + 2HSO_4^-(aq) ----> 2PbSO4(s) + 2H2O(l)$

Calculate  E at 25°C for this battery when [H2SO4] = 5.0 M; that is, [H + ] = [HSO4− ] = 5.0 M. At 25°C,  E° = 2.04 V for the lead storage battery.

Answer:

The  voltage of the cell is  $E = 2.12V$

Explanation:

 From the question we are told that

          The original voltage of the battery is $E = 2.04 V$

           The concentration of  [H2SO4] = 5.0 M

            The concentration of  [H + ] = [HSO4− ] = 5.0 M

At equilibrium

                   The reaction quotient is  

                                             $Q = \frac{1}{[[HSO_4^-]^2 [H^+] ^2]}$

Pb(s), Pb(s), 2 H2O(l),2 PbSO4(s) are excluded from the reaction above because they are solid and liquid thus there concentration does not change

                 $Q = \frac{1}{5^2 * 5^2}$

                    $= 1.6*10^{-3}$

So the potential for the battery cell is mathematically evaluated as

             $E = E^o - \frac{0.05916}{2} log Q$

                      $= 2.04 - [\frac{0.05916}{2} log (1.6*10^{-3})]$

             $E = 2.12V$

                         

Answer 2

Answer:

2.12 V

Explanation:

see attached file for the detailed step by step solution of the given problem.