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 does the internal energy of the gas change?
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) of a system is equal to the heat (Q) added to the system minus the work (W) done by the system:
ΔU = Q - W
Given that 820 kJ of energy are transferred to the gas and 100 kJ of work are done on the gas, 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 the internal energy of the gas can be calculated using the First Law of Thermodynamics, which states that the change in internal energy of a system is equal to the heat transferred to the system minus the work done by the system.
Given:
Heat transferred to the gas, Q = 820 kJ
Work done on the gas, W = 100 kJ
Using the First Law of Thermodynamics:
Change in internal energy (ΔU) = Q - W
Substituting the given values:
ΔU = 820 kJ - 100 kJ
ΔU = 720 kJ
Thus, the internal energy of the gas changes by 720 kJ.