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 3.20 mol of H2 with 1.60 mol of O2 at atmospheric pressure if the volume change is - 22.6L?

Express your answer using three significant figures

Question

Chemistry

Keaton Owen

27 June, 14:42

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 3.20 mol of H2 with 1.60 mol of O2 at atmospheric pressure if the volume change is - 22.6L?

Express your answer using three significant figures

+5

Answers (1)

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Raina · Answer 1

The work done * on * a system that undergoes an infinitesimal volume change, dV under the influence of an * external * pressure of p is given by:

δw = - p dV

If p is constant, this integrates to:

w = - p*ΔV

In this case,

w = - (101325 Pa) * (-7.3 L) (1m3/1000L) = 2289.945 J