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What is the balanced redox reaction for the combustion of methane (CH4) in the presence of oxygen (O2) to form carbon dioxide (CO2) and water (H2O)?
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Feb 17
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Chemical reactions
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CharleyPrior
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What is the balanced redox reaction for the combustion of methane (CH4) in the presence of oxygen (O2) to form carbon dioxide (CO2) and water (H2O)?
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Feb 17
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ChadLarocque
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The balanced redox reaction for the combustion of methane CH4 in the presence of oxygen O2 to form carbon dioxide CO2 and water H2O is as follows:CH4 + 2 O2 CO2 + 2 H2O
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Here's a precise problem for a chemistry student to solve:Using Hess's Law, calculate the enthalpy change for the reaction where 2 moles of methane (CH4) reacts with 4 moles of oxygen gas (O2) to form 2 moles of carbon dioxide (CO2) and 4 moles of water (H2O), given the following known enthalpy changes:ΔH1 = -890 kJ/mol for the reaction: CH4 + 2O2 → CO2 + 2H2OΔH2 = -394 kJ/mol for the reaction: C + O2 → CO2ΔH3 = -286 kJ/mol for the reaction: H2 + (1/2)O2 → H2O
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Calculate the enthalpy change for the combustion of methane gas (CH4) at standard conditions given the following information: 4 moles of methane gas is burned in excess oxygen gas (O2) to form carbon dioxide gas (CO2) and liquid water (H2O). The enthalpy change for the combustion of 1 mole of methane gas is -890.4 kJ/mol.
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