If a system absorbs 500 cal of heat at the same time does 400J of work, find the change in internal energy of the system.
Answered Feb 05, 2023
ΔU = q + w (1 Calorie =4.2 J) ΔU = 2100+(-400) = 1700J
(d) : It does not violate first law of thermodynamics but violates second law of thermodynamics.
(c) the temperature of a body can be increased by doing work on it
The correct answer is (a) (d) (a) The process must be adiabatic. (d) The temperature must decrease.
Q = 100J We know, ΔU = ΔQ – ΔW Here since the container is rigid, ΔV = 0, Hence the ΔW = PΔV = 0, So, ΔU = ΔQ = 100J.
ΔU = q + w ΔU = 802 + (-294) =508J
ΔU Decreases. (ΔU = q - w)
ΔU increases. (ΔU = q + w)
Δ U = w , wall is adiabatic
Δ U = - q, thermally conducting walls
Δ U = q – w, closed system
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