Question

The combustion of methane gas (ch4) forms co2(g) h2)(l). calculate the heat produced by burning 1.85 mol of the methane gas.

use these delta change h zero f data to help: ch4(g)=-74.9 kj/mol, co2(g)=-393.5 kj/mol, h2o(l)=-285.8 kj/mol. answer in units of kj.

Answer 1

The combustion of 1.85 mol of methane gas (CH4) produces 1647.24 kJ of heat energy, based on the thermochemical equation which indicates that 890.4 kJ is released per mole of methane combusted.

Step-by-step explanation:

To calculate the heat produced by the combustion of methane, we use the given enthalpy of formation (ΔH°f) values and the amount of methane burned. The thermochemical equation for the combustion of methane is:

CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l) + 890.4 kJ

This equation indicates that for every mole of methane combusted, 890.4 kJ of heat is released. Since we are given that the combustion of 1.85 mol of methane needs to be calculated, we multiply the amount of heat released by one mole by the given number of moles:

Heat released = 890.4 kJ/mol × 1.85 mol

The result is:

Heat released = 1647.24 kJ

Therefore, the combustion of 1.85 mol of methane gas produces 1647.24 kJ of heat energy.