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# Problem: A mole of X reacts at a constant pressure of 43.0 atm via the reactionX(g)+4Y(g)=&gt;2Z(g) ΔH=-75.0 kJBefore 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.

###### FREE Expert Solution

Calculate ΔE:

$\overline{){\mathbf{∆}}{\mathbf{E}}{\mathbf{=}}{\mathbf{q}}{\mathbf{+}}{\mathbf{w}}}$

At constant pressure, the heat of reaction (q) is equal to the enthalpy change (ΔH) of the system.

q = ΔH = -75.0 kJ

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###### Problem Details

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.