The following chemical reaction occurs in a car battery:

$P{b}_{(c)}+Pb{O}_{2(a)}+2H_{2}S{O}_{4(aq)}2PbS{O}_{4(c)}+2H_2{O}_{(l)}$

Given the following enthalpy of formation values, calculate the enthalpy change for the above reaction as written

$($enthalpy of reaction$)($Ans: $-315\mathrm{.}6kJ)$

$Pb{O}_{2(d)},H_{2}S{O}_{4(nq)},PbS{O}_{4(l)},H_2{O}_{(l)}$

$-277\mathrm{.}0k\frac{J}{m}ol,-909\mathrm{.}3k\frac{J}{m}ol,-902\mathrm{.}1k\frac{J}{m}ol,-285\mathrm{.}5k\frac{J}{m}ol$

b$)$ If it takes $39\mathrm{.}5kJ$ to start your car, what mass of lead $($II$)$ sulphate is produced when starting the car using the

battery reaction described in $\text{'}$a$\text{'}?($Ans: $75\mathrm{.}8$g$)$