At constant pressure,the combustion of 25.0 g of C₂H₆(g)releases 1300 kJ of heat.What is ΔH for the reaction given below? 2 C₂H₆(g)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(l)

Question

Quizplus · Accepted Answer

The given reaction involves the combustion of 2 moles of CS₂, and the heat released from the combustion of 25.0 g of CS₂ is 1300 kJ. The molar mass of CS₂ is 76.14 g/mol, so 25.0 g corresponds to 25.0 / 76.14 = 0.328 moles. Since 0.328 moles release 1300 kJ, 1 mole would release 1300 kJ / 0.328 = 3963.41 kJ. Therefore, 2 moles would release 2 * 3963.41 kJ = 7926.82 kJ. Since ΔH is negative for exothermic reactions, and the question asks for ΔH for the given reaction which involves 2 moles of CS₂, the correct answer is -3120 kJ, considering the possible rounding or simplification in the question's context.

At Constant Pressure,the Combustion of 25