One mole of ideal gas is heated to raise temperature by 1°C at constant P and constant V. Difference in work done in the two cases will be equal to :2 cal8.314 cal08.21 L atm
Question
One mole of ideal gas is heated to raise temperature by 1°C at constant P and constant V. Difference in work done in the two cases will be equal to :2 cal8.314 cal08.21 L atm
Solution
The work done on a system at constant pressure and constant volume 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 added to the system minus the work done by the system.
At constant volume (V), no work is done because the volume is not changing. Therefore, the work done (W) is zero.
At constant pressure (P), the work done can be calculated using the formula W = PΔV, where ΔV is the change in volume. However, we are not given the change in volume in this problem.
The difference in work done in the two cases would be the work done at constant pressure minus the work done at constant volume. Since the work done at constant volume is zero, the difference in work done is just the work done at constant pressure.
Without the change in volume, we cannot calculate the exact value of the work done at constant pressure. Therefore, we cannot determine the difference in work done in the two cases based on the information given in the problem.
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