Chapter 8, Problem 63QAP

Butane gas, C₄H₁₀, is sold to campers as bottled fuel. Its density at 25°C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25°C and 1.00 atm is required to heat one gallon of water $\left(d=1.00\text{g}/\text{mL}\right)$ from 25°C to 98°C ? The reaction for the combustion of butane $\left(\Delta H_{\text{f}}{}^{°}=-125.6\text{kJ}/\text{mol}\right)$ is

${\text{C}}_{\text{4}}{\text{H}}_{\text{1}0}\left(g\right)+\frac{13}{2}{\text{O}}_{\text{2}}\left(g\right)\to {\text{4CO}}_{\text{2}}\left(g\right)+{\text{5H}}_{\text{2}}\text{O}\left(g\right)$