Reacting 10.0 mL of H2(g) with 10.0 mL of C2H4(g) produces 10.0 mL of C2H6 at 1.5 atm. If the reaction produces 3.1 kJ of heat and the decrease in volume requires the heat surroundings do 7.6 J of work on the gases, what is the change in internal energy of the gases?
Q = -3.1 KJ = -3100 J
Negative because heat is lost from the mixture
W = + 7.6 J
Positive because work is done on the mixture.
Use:
Delat E = Q + W
= -3100 J + 7.6 J
= -3092.4 J
= -3.0924 KJ
Answer: -3.0924 KJ
Reacting 10.0 mL of H2(g) with 10.0 mL of C2H4(g) produces 10.0 mL of C2H6 at 1.5 atm. If the reaction produces 3.1 kJ o...
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