The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ:2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJHow much PV work is done in kilojoules for the reaction of 0.28 mol of H2 with 0.14 mol of O2 at atmospheric pressure if the volume change is -7.7 L?What is the value of ΔE in kilojoules?
The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ:
2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ
How much PV work is done in kilojoules for the reaction of 0.28 mol of H2 with 0.14 mol of O2 at atmospheric pressure if the volume change is -7.7 L?
What is the value of ΔE in kilojoules?
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