MHT CET · Chemistry · Thermodynamics (C)

Two moles of an ideal gas are allowed to expand from a volume of $10 d m^{3}$ to $2 m^{3}$ at $300 K$ against a pressure of $101.325 K P a.$ Calculate the work done.

A $- 201.6 k J$
B $13.22 k J$
C $- 810.6 k J$
D $- 18.96 k J$

Verified Solution

Answer & Solution

Correct Answer

(A) $- 201.6 k J$

Step-by-step Solution

Detailed explanation

V_{1} = 10 {dm}^{3} = 1 0^{- 2} m^{3}

V_{2} = 2 m^{3}

V_{2} - V_{1} = (2 - 10^{- 2})

= 1.99 m^{3}

P = 101.325 \times 1 0^{3} pa

W = - P_{e x t} . Δ V

W = - 101.325 \times 1 0^{3} (1.99)

= 201.6 k J

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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Two moles of an ideal gas are allowed to expand from a volume of 10 dm3 to 2 m3 at 300 K against a pressure of 101.325 KPa. Calculate the work done.

Step-by-step Solution

Two moles of an ideal gas are allowed to expand from a volume of $10 d m^{3}$ to $2 m^{3}$ at $300 K$ against a pressure of $101.325 K P a.$ Calculate the work done.