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Rapid oxidation of a substance, accompanied by the production of heat and light.
3. Chemical Reactions
Combustion Analysis
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Calculate the enthalpy change (ΔH) for the combustion of propane gas (C3H8) when water is produced as a gas, given that ΔH_comb for the formation of liquid water is -2219 kJ/mol and the enthalpy of vaporization (ΔH_vap) for water is +44 kJ/mol.
A
-2175 kJ/mol
B
-2263 kJ/mol
C
-2219 kJ/mol
D
-2263 kJ/mol
Verified step by step guidance1
Write the balanced chemical equation for the combustion of propane (C3H8). The combustion reaction involves propane reacting with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).
Identify the enthalpy change for the formation of liquid water (ΔH_comb) and the enthalpy of vaporization (ΔH_vap) for water. These values are given as -2219 kJ/mol and +44 kJ/mol, respectively.
Calculate the enthalpy change for the formation of gaseous water by adding the enthalpy of vaporization to the enthalpy change for the formation of liquid water. Use the formula: ΔH_gas = ΔH_comb + ΔH_vap.
Determine the total enthalpy change for the combustion of propane by considering the stoichiometry of the balanced equation. Multiply the enthalpy change for the formation of gaseous water by the number of moles of water produced in the reaction.
Sum the enthalpy changes for all products and reactants to find the overall enthalpy change (ΔH) for the combustion of propane. Ensure that the sign of ΔH reflects the exothermic nature of the combustion process.
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