The combustion of 1.00 mole of methane, CH4, produces carbon dioxide and water and releases 802 kJ•mol–1. When 3.00 mol of oxygen react with a stoichiometric quantity of methane, what is ΔH for the reaction?
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Help!
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CH4 + 2 O2 → CO2 + 2 H2O
According to the balanced equation above, 1 mole of CH4 reacts with 2 moles of O2 to produce 1 mole of CO2 and 2 moles of H2O.
1 mole of CH4 reacts with 2 moles of O2, so x moles of CH4 reacts with 3 moles of O2. Set up a proportion and solve for x.
1 / 2 = x / 3, x = 1.5 moles of CH4
When 1 mole of CH4 is burned, it releases 802 kJ of heat energy. When 1.5 mole of CH4 is burned, it releases 1.5 * 802 kJ of heat energy.
ΔH = 1203 kJ of heat energy
The mole ratio, in the balanced equation, determines the answers in stoichiometry problems!
According to the balanced equation above, 1 mole of CH4 reacts with 2 moles of O2 to produce 1 mole of CO2 and 2 moles of H2O.
1 mole of CH4 reacts with 2 moles of O2, so x moles of CH4 reacts with 3 moles of O2. Set up a proportion and solve for x.
1 / 2 = x / 3, x = 1.5 moles of CH4
When 1 mole of CH4 is burned, it releases 802 kJ of heat energy. When 1.5 mole of CH4 is burned, it releases 1.5 * 802 kJ of heat energy.
ΔH = 1203 kJ of heat energy
The mole ratio, in the balanced equation, determines the answers in stoichiometry problems!