Finding Work with constant pressure and temp.

[phizzle86]

The conversion of propene (C3H6) to dichloromethane (CH2Cl2) takes place according to the
reaction
C3H6(g) + 3Cl2(g) 6 3CH2Cl2(g).
At 298.15 K, the standard enthalpy change of this reaction is -306.98 kJ mol-1 and the
standard enthalpy of formation of CH2Cl2(g) is -95.52 kJ mol-1.

Calculate q, w, deltaU, and deltaH for the production of one mole of CH2Cl2(g) by this reaction
at a constant pressure of one bar and a temperature of 298.15 K.



I'm having trouble finding the work done, how can you determine the work done if there's no change in volume? Please help (A: w=826 J)

Thank you.

 

[Spinnor]

If the volume changes at constant pressure work is done. Work = pressure X area X distance = pressure X volume