Chapter 6.3, Problem 6.4E

Consider the combustion (burning) of methane, CH₄, in oxygen.

${\text{CH}}_4(g)+2{\text{O}}_2(g)\to {\text{CO}}_2(g)+2{\text{H}}_2\text{O}(l)$

The heat of reaction at 77°C and 1.00 atm is −885.5 kJ. What is the change in volume when 1.00 mol CH₄ reacts with 2.00 mol O₂? (You can ignore the volume of liquid water, which is insignificant compared with volumes of gases.) What is w for this change? Calculate ΔU for the change indicated by the chemical equation.