Question

I am stuck on b)...

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 heat evolved,c) the change in internal energy of the system, and d) the change in internal energy of the surroundings.

My answers:
a) w= 2.27 x10^3 J Is this correct?
b) Is this set up correct?
Heat evolved:
q=(67,200g)x(4.184J/gC)x(273K)=..
I am not sure what is the temperature change...
c) dE=q+w.. But I need part b) checked before I can do part c) correctly..
d) Would the answer for part d) be the same as part c) but with different sign?

Answer 1

C2H2 + H2 ==> C2H4 + 6.3 kJ
I don't know how you obtained that answer for a.
Isn't be just 6.3 kJ?
As for the T change, the problem states it is STP at the beginning and is maintained at STP.
As for your calculation for b, how did the specific heat H2O get in there.?