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A mole of XX reacts at a constant pressure of 43.0 atmatm via the reaction X(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJX(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 LL. After the reaction, the volume was 2.00 LL. Calculate the value of the total energy change, ΔE, in kilojoules.

A mole of XX reacts at a constant pressure of 43.0 atmatm via the reaction X(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJX(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 LL. After the reaction, the volume was 2.00 LL. Calculate the value of the total energy change, ΔE, in kilojoules.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 64QRT
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A mole of XX reacts at a constant pressure of 43.0 atmatm via the reaction

X(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJX(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJ

Before the reaction, the volume of the gaseous mixture was 5.00 LL. After the reaction, the volume was 2.00 LL. Calculate the value of the total energy change, ΔE, in kilojoules.

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