When 2.00 kJ of energy is transferred as heat to nitrogen in a cylinder fitted with a piston with an external pressure of 2.00 a
tm, the nitrogen gas expands from 2.00 to 5.00 L. What is the change in internal energy of this system? (1 L·atm = 0.1013 kJ)
1 answer:
Answer:
ΔU= 1.3922 KJ
Explanation:
Given that
Q= 2 KJ
Note- 1 .Heat added to the system taken as positive and heat leaving from the system is taken negative.
2. Work done on the system taken as negative and work done by the system taken as positive.
P =2 atm
V₁= 2 L
V₂=5 L
Work done by the gas W
W= P ( V₂- V₁)
W= 2 ( 5 - 2)
W= 6 atm.L
1 L·atm = 0.1013 kJ
W= 0.6078 KJ
From first law of thermodynamics
Q= W + ΔU
ΔU=Change in internal energy
2 = 0.6078 + ΔU
ΔU= 1.3922 KJ
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