Reacting 1 L of H2(g) with 1 L C2H2(g) (both at STP) results in the formation of 1 L of C2H4(g) if the reaction is maintained at the same conditions (STP) and goes to completion. If this reaction produced 6.3 kJ of heat (absorbed by the surroundings), calculate: a) the PV work and b) the change in internal energy of the system.

Question

Reacting 1 L of H2(g) with 1 L C2H2(g) (both at STP) results in the formation of 1 L of C2H4(g) if the reaction is maintained at the same conditions (STP) and goes to completion. If this reaction produced 6.3 kJ of heat (absorbed by the surroundings), calculate: a) the PV work and b) the change in internal energy of the system.

I got w= -2.27 x10^3 J.
Is this correct?
If so, I will proceed to the next question and have you check it...
I think if I calculate w wrong, the other answers will be wrong as well so..

Answer 1

I don't understand how you obtained this value for work.

P is 1 atm (STP) and delta V is 1L. Right?