Multiple Choice
What is the standard enthalpy change for the combustion of one mole of benzene (C6H6) based on the given reaction: 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(l); ΔHrxn° = -6534 kJ?
3. Chemical Reactions
Combustion Analysis
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When 0.112 g of heptene, C7H14, is burned in a bomb calorimeter, the temperature rises by 4.99 °C. The heat capacity of the calorimeter is 2.46 kJ/°C. Calculate the combustion energy (ΔE) for heptene, C7H14, in kJ/mol. Express your answer in kJ/mol.
A
-5000 kJ/mol
B
-4180 kJ/mol
C
-2500 kJ/mol
D
-3500 kJ/mol
Verified step by step guidance1
Identify the given values: mass of heptene (0.112 g), temperature change (4.99 °C), and heat capacity of the calorimeter (2.46 kJ/°C).
Calculate the total heat absorbed by the calorimeter using the formula: q = C_calorimeter × ΔT, where C_calorimeter is the heat capacity and ΔT is the temperature change.
Convert the mass of heptene to moles using its molar mass. The molar mass of heptene (C7H14) can be calculated by adding the atomic masses of its constituent atoms.
Determine the combustion energy per mole of heptene by dividing the total heat absorbed by the number of moles of heptene. Use the formula: ΔE = q / moles of heptene.
Express the combustion energy in kJ/mol, ensuring the sign reflects the exothermic nature of the reaction (negative sign).
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