A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.00^ . As it does so, it absorb - Chemistry MCQ JEE Main 2026 | ExamTest.live

mediumMCQJEE Main2026Chemistry

1 mark

A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0 0^{\circ} C . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be (R = 8.314 J/mol K):

Solution & Step-by-step Explanation

For an isothermal process (Δ T = 0) involving an ideal gas:Internal energy change Δ U = n C_{v} Δ T = 0 .From the First Law of Thermodynamics: Δ U = q + w .Since Δ U = 0, q = - w .The gas absorbs 208 J of heat, so q = + 208 J .Therefore, w = - 208 J .

Try it yourself before checking the explanation above.

A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0 0^{\circ} C . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be (R = 8.314 J/mol K):

q = - 208 J, w = - 208 J

q = - 208 J, w = + 208 J

q = + 208 J, w = + 208 J

q = + 208 J, w = - 208 J

Practice with timed mock tests and track your performance across Chemistry.