Question

How much heat is released when 6.00 g of methane is combusted using the reaction below?

CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (l) △H = -890.0 kJ

Answer 1

To calculate the heat released from the combustion of 6.00 g of methane, convert the mass to moles using methane's molar mass and then use the thermochemical equation to find that 6.00 g of methane releases 332.86 kJ of heat.

Step-by-step explanation:

The amount of heat released when 6.00 g of methane is combusted can be found by using stoichiometry based on the given thermochemical equation CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) ΔH = -890.0 kJ. This equation states that the combustion of 1 mol of methane (CH4) releases 890.0 kJ of heat energy.

To determine the heat released by 6.00 g of methane, we must first convert the mass of methane to moles using the molar mass of methane (16.04 g/mol):

1. 6.00 g CH4 × (1 mol CH4 / 16.04 g CH4) = 0.374 mol CH4

Next, we calculate the heat released using the molar ratio from the thermochemical equation:

1. 0.374 mol CH4 × (890.0 kJ / 1 mol CH4) = 332.86 kJ

Therefore, the combustion of 6.00 g of methane releases 332.86 kJ of heat.