The gas received an amount of heat equal to 300 J and performed work equal to 400 J. How did the internal energy of the gas change, if its mass is constant?
According to the first law of thermodynamics:
∆U = Q + A ‘, where Q is the amount of heat that was received – given the gas (Q> 0 and Q = 300 J, since heat is supplied to the system), ∆U is the change in the internal energy of the gas, A’ is the perfect work gas – over the gas (A ‘<0, A’ = -400 J, since the work was done by the system).
Let’s calculate the change in the internal energy of the gas:
∆U = Q + A ‘= 300 + (-400) = 300 – 400 = -100 J.
Answer: The internal energy of the gas decreased by 100 J.
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