A cylinder contains 3 moles of oxygen at a temperature of `27^(@)C`. The cylinder is provided with a frictionless piston which maintains a constant pressure of 1 atm on the gas. The gas is heated until its temperature rises to `127^(@)C`.
a. How much work is done by the gas in the process ?
b. What is the change in the internal energy of the gas ?
c. How much heat was supplied to the gas ?
For oxygen `C_(P) = 7.03 cal mol^(-1) .^(@)C^(-1)`.

Explanation

Let's solve the problem step by step.

### Given Data:
- Number of moles of oxygen, \( n = 3 \, \text{moles} \)
- Initial temperature, \( T_1 = 27^\circ C = 300 \, K \)
- Final temperature, \( T_2 = 127^\circ C = 400 \, K \)
- Constant pressure, \( P = 1 \, \text{atm} \)
- Heat capacity at constant pressure for oxygen, \( C_P = 7.03 \, \text{cal mol}^{-1} \, ^\circ C^{-1} \)
...