To determine the change in internal energy of the gas during the expansion, we need to consider the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
Mathematically, this can be represented as:
ΔU = Q - W
Where:
ΔU = Change in internal energy
Q = Heat added to the system
W = Work done by the system
In this case, the cylinder of gas does 970 J of work on the piston, indicating that work is being done by the gas. Therefore, W = -970 J.
The gas also transfers 620 J of energy to the piston and the outside system, which indicates that heat is being added to the gas. Therefore, Q = +620 J.
Plugging these values into the equation:
ΔU = Q - W
ΔU = 620 J - (-970 J)
ΔU = 620 J + 970 J
ΔU = 1590 J
Therefore, the internal energy of the gas changes by 1590 J during this expansion.
A cylinder of gas does 970j of work on a piston. The gas also transfer 620j of energy to the piston and outside system while it expands. How much does the internal energy of the gas change during this expansion?
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