Two moles of an ideal gas initially at `27^(@)C` and one atmospheric pressure are compressed isothermally and reversibly till the final pressure of the gas is 10 atm calculate q, w and `Deltaw` for the process

Explanation

To solve the problem step by step, we will calculate the heat transfer (q), work done (w), and the change in internal energy (ΔU) for the isothermal and reversible compression of the ideal gas.

### Step 1: Identify the Given Data
- Number of moles (n) = 2 moles
- Initial temperature (T) = 27°C = 300 K (convert to Kelvin by adding 273)
- Initial pressure (P1) = 1 atm
- Final pressure (P2) = 10 atm
- Ideal gas constant (R) = 8.314 J/(mol·K)
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