A gas is placed next to a reservoir of a higher temperature. The reservoir thus transfer 820kj of energy to the gas. 100kj of work are also done on this gas. By how much the internal energy of the gas changes?
The change in the internal energy of the gas can be determined by the first law of thermodynamics, which states that the change in internal energy (ΔU) is equal to the heat transfer (Q) to the gas minus the work done (W) on the gas.
ΔU = Q - W
Given that the reservoir transfers 820 kJ of energy to the gas (Q = 820 kJ) and 100 kJ of work are done on the gas (W = 100 kJ), we can substitute these values into the equation:
ΔU = 820 kJ - 100 kJ
ΔU = 720 kJ
Therefore, the internal energy of the gas changes by 720 kJ.
The change in internal energy of the gas can be calculated using the first law of thermodynamics, which states that the change in internal energy (ΔU) is equal to the heat (Q) supplied to the gas minus the work (W) done on the gas.
Mathematically, the equation is:
ΔU = Q - W
Given that the reservoir transfers 820 kJ of energy to the gas (Q = 820 kJ) and 100 kJ of work is also done on the gas (W = 100 kJ), we can substitute these values into the equation to find the change in internal energy.
ΔU = 820 kJ - 100 kJ
ΔU = 720 kJ
Therefore, the internal energy of the gas changes by 720 kJ.