At constant pressure,the combustion of 20.0 g of C₂H₆(g)releases 1036 kJ of heat.What is ΔH for the reaction given below? 2 C₂H₆(g)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(l) A) -86.1 kJ B) -781 kJ C) -1600 kJ D) -3120 kJ

Question

Quizplus · Accepted Answer

The given reaction involves the combustion of 2 moles of CS2, and the heat released from the combustion of 20.0 g of CS2 is 1036 kJ. The molar mass of CS2 is approximately 76.14 g/mol, so 20.0 g corresponds to 20.0 g / 76.14 g/mol ≈ 0.263 moles of CS2. Since 0.263 moles release 1036 kJ, 1 mole would release 1036 kJ / 0.263 ≈ 3940 kJ. Therefore, 2 moles would release 2 * 3940 kJ = 7880 kJ. Since the reaction is exothermic, ΔH is negative, making ΔH = -7880 kJ for the combustion of 2 moles of CS2. However, none of the provided options match this calculation directly, suggesting a misunderstanding in the calculation process or an error in interpreting the question's requirements. Given the options, the closest approach to a logical answer based on the provided information and standard stoichiometric and thermochemical calculations would be to reassess the calculation or the interpretation of the question's data and intent.

At Constant Pressure,the Combustion of 20