Two moles of an ideal gas was heated isobarically so that its temperature was raised by 100 K. The heat absorbed during the process was 4000 J. Calculate (i) the work done by the gas, (ii) the increase in internal energy and (ii) the value of y for the gas `[R =8.31 J mol ^(-1) K ^(-1) ].`

Explanation

To solve the problem step by step, we will calculate the work done by the gas, the increase in internal energy, and the value of \( \gamma \) (gamma) for the gas.

### Given Data:
- Number of moles, \( n = 2 \) moles
- Temperature change, \( \Delta T = 100 \) K
- Heat absorbed, \( Q = 4000 \) J
- Universal gas constant, \( R = 8.31 \, \text{J mol}^{-1} \text{K}^{-1} \)

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