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 3 7 . 0 ∘ 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) (ln7.5 = 2.01)

Question

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 3 7 . 0 ∘ 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) (ln7.5 = 2.01), q = - 2 0 8 J , w = + 2 0 8 J, q = + 2 0 8 J , w ⁡ = + 2 0 8 J, q = + 2 0 8 J , w ⁡ = - 2 0 8 J, q = - 2 0 8 J , w ⁡ = - 2 0 8 J

MARKS App · Accepted Answer

Since, temperature remains constant, the process will be isothermal by nature. For Isothermal reversible expansion: Δ E = 0 = q + w q = - w q = + 2 0 8 J {heat absorbed so +ve} w = - 2 0 8 J {expansion so work done is -ve}

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