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The reaction between hydrogen and oxygen to yield water vapor has ΔH∘ = -484 kJ:2H2(g) O2(g) → 2H2O(g) ΔH∘ = -484 kJA) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol of O2 at atmospheric pressure if the volume change is -3.8 L?B) What is the value of ΔE in kilojoules?
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