Question

In the following reaction how much heat is generated when 5.95 moles of CH four are burned? Ch4 (g) + 2 O2 (g)—> CO2 (g) + 2 H2O (g) $\Delta$ H = -802 kJ/mol

Answer 1

$CH_4+2O_2\to CO_2+2H_2O \Delta H=-802kJ/Mol$

One mole is equivalent to -802kJ of heat.

Heat generated when 5.95 moles of $CH_4$ are burned $=5.95\times (-802)=-4771.9kJ$