Question

In the following reaction, what is the quantity of heat (in kJ) released when 2.07 moles of CH‚„ are burned? CH‚„ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ΔH° = -802 kJ/mol

Answer 1

When 2.07 moles of CH4 are burned, 1842.128 kJ of heat is released according to the thermochemical equation for the combustion of methane.

Step-by-step explanation:

The student has asked about the quantity of heat released when burning 2.07 moles of CH4. The balanced thermochemical equation for the combustion of methane (CH4) is as follows:

CH4(g) + 2 O2 (g) → CO2 (g) + 2 H2O(l) ΔH° = -890.4 kJ/mol

According to the equation, the combustion of 1 mole of CH4 releases 890.4 kJ of heat. To find the heat released for 2.07 moles, we multiply the heat released per mole by the number of moles:

(890.4 kJ/mol) × (2.07 mol) = 1842.128 kJ

Hence, the quantity of heat released when 2.07 moles of CH4 are burned is 1842.128 kJ.