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?
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.
To determine how much the internal energy of the gas changes during this expansion, we need to use the First Law of Thermodynamics.
According to the First Law of Thermodynamics, the change in internal energy of a system is equal to the heat added to the system minus the work done by the system:
ΔU = Q - W
Given:
Work done by the gas on the piston (W) = 970 J
Energy transferred to the piston and outside system (Q) = 620 J
Now, substitute the given values into the equation:
ΔU = Q - W
ΔU = 620 J - 970 J
ΔU = -350 J
Therefore, the internal energy of the gas changes by (-350 J) during this expansion.