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A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules. Express your answer with the appropriate units.

Respuesta :

Thank you for posting your question here at brainly. I hope the answer will helps. Below is the solution:

(4.18 J/(g⋅∘C)) x (35.0 g + 2.10 g) x (27.5 - 13.0)∘C = 2248.6 J gained by the solution 

(2248.6 J) / (2.10 g / (80.0 g/mol)) = 85661 J/mol = 85.7 kJ/mol

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