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Answer :
To calculate the heat released by the combustion of 97.7g of CH4, first convert the mass of methane to moles. The ΔH of methane is -890.3 kJ/mol. The total energy released is approximately 5432.3 kJ.
To calculate the heat released by the combustion of 97.7g of CH4 (methane), you first need to know the enthalpy change of the reaction (ΔH), also known as heat of combustion. The heat of combustion of methane is -890.3 kJ/mol.
Step 1: Convert the mass of methane to moles. CH4 has a molecular weight of approximately 16 g/mol. So, 97.7g of CH4 is equivalent to 97.7g ÷ 16g/mol = 6.10625 mol.
Step 2: Calculate the total heat released. Since the ΔH of methane is the energy released per mol, total energy released will be 6.10625 mol × -890.3 kJ/mol = -5432.30375 kJ. The negative sign indicates that the energy is being released, not absorbed.
So approximately 5432.3 kJ of heat will be released when 97.7g of CH4 combusts.
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