[student8607]

The reaction between hydrogen and oxygen to yield water vapor has  :delta: H = -484kJ

2H₂(g) + O₂(g) --> 2 H₂O(g)

How much PV work is done and what is the value of  :delta: E in kJ for the reaction of 0.50mol of H₂ with 0.25mol of O at atmospheric pressure if the volume change is -5.6L


The only equation I am familiar with is:  :delta: E =  :delta: H - P :delta: V
But I don't know how to account for moles of the reactants.