A 5.0 mole sample of ideal gas is heated reversibly at constant pressure (2.5 at

Question

A 5.0 mole sample of ideal gas is heated reversibly at constant pressure (2.5 atm) from 300. K to 750. K. Assume the gas has a constant pressure heat capacity. C_p = 5/2 R. Calculate the work done. Calculate the heat flow. Calculate the delta U for this process. Calculate the delta H for this process. A 3.48 mole sample of CO at 350. K and 100. L is compressed isothermally and reversibly to 25 L. Assume C_p = 7/2 R. Calculate the work done. Assuming CO to be an ideal gas, where delta U = 5/2 RT. calculate delta U for this process. Calculate q for this process.

Explanation / Answer

(6)

initial volume of gas = nRT/P = ( 5 mol x 0.082 x 300 K ) / 2.5 atm == 49.2 L

Final volume of gas = nRT2/P == ( 5 mol x 0.082 x 750 K ) / 2.5 atm == 123 L

(a)

work done = nR(T2-T1) = 5 mol x 8.314 x(750-300) == 31.18 kJ

(b)

Heat Flow= nCpdT = 5 mol x (5/2*8.314) x (750-300) = 77.94 kJ

(c) dU = dH +pdV = dH - dW == 77.94 kJ - 31.18 kJ = 46.76 kJ

(d) for constant pressure process, q = delta H

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