Chapter 5, Problem 5.35QE

The thermochemical equation for the burning of methane, the main component of natural gas, is

$\begin{array}{l}{\text{CH}}_{\text{4}}\left(\text{g}\right)+2{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{CO}}_{\text{2}}\left(\text{g}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\mathcal{l}\right)\\ \Delta H=-890\text{kJ}\end{array}$

(a) Is this reaction endothermic or exothermic?

(b) What quantities of reactants and products are assumed if ΔH = –890 kJ?

(c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?