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Given that U = (3/2)PV does this mean that ΔU = Δ(3/2)PV for an ideal gas? Hence when finding the change in internal energy using a P-V diagram, can we simply apply this equation instead of using ΔU = Q+W?
The change in internal energy of an ideal gas refers to the difference between the initial and final internal energies of the gas. It is a measure of the energy transferred to or from the gas in the form of heat or work.
The change in internal energy of an ideal gas can be calculated using the equation ΔU = Q - W, where ΔU is the change in internal energy, Q is the heat added to the gas, and W is the work done by the gas.
The change in internal energy of an ideal gas is affected by the amount of heat added or removed, the work done on or by the gas, and the initial and final temperatures of the gas.
No, the change in internal energy of an ideal gas can be positive or negative. A positive change indicates an increase in the internal energy of the gas, while a negative change indicates a decrease in internal energy.
The change in internal energy of an ideal gas is important in understanding the thermodynamic properties of gases and their behavior. It is also a key factor in determining the efficiency of heat engines and other thermodynamic processes.