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

To solve the problem step by step, we will calculate the work done by the gas, the change in internal energy, and the heat supplied to the gas.

### Given Data:
- Number of moles of oxygen (n) = 3 moles
- Initial temperature (T1) = 27°C = 300 K (convert to Kelvin by adding 273)
- Final temperature (T2) = 127°C = 400 K (convert to Kelvin)
- Constant pressure (P) = 1 atm
- Specific heat at constant pressure (Cₚ) = 7.03 cal/mol/°C
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