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(a) What sign for ∆S do you expect when the volume of 0.200 mol of an ideal gas at 27 °C is increased isothermally from an initial volume of 10.0 L? (b) If the final volume is 18.5 L, calculate the entropy change for the process. (c) Do you need to specify the temperature to calculate the entropy change? Explain.

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Collen Von
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23 May 2020

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Related questions

(a) What sign for ∆S do you expect when the pressure on 0.600 mol of an ideal gas at 350 K is increased isothermally from an initial pressure of 0.750 atm? (b) If the final pressure on the gas is 1.20 atm, calculate the entropy change for the process. (c) Do you need to specify the temperature to calculate the entropy change? Explain.

15.0 g of CH4 (g) is expanded isothermally at 260 K from an initial pressure of 150 kPa to a final pressure of 105 kPa. Calculate the change in entropy for the gas and the change in entropy for the gas, assuming the expansion is performed (A) reversibly and (B) irreversibly.

This problem asks for the change in entropy along various pathways. Use heat capacities from the end flap or quick reference pages of the Elliott and Lira textbook, assuming they are independent of T.

(CP/R) = 3.505

Note the tabulated value is Cp/R. Multiply by R to get Cp in the desired units.

You can find V using the ideal gas law.

(a) Gaseous carbon monoxide is heated isobarically at 0.7 MPa from 300 K to 405 K. What is the change in entropy (J/mol-K)?

(b) Gaseous carbon monoxide is compressed isothermally at 405 K from 0.7 MPa to 5.5 MPa. What is the change in entropy (J/mol-K)?

(c) Gaseous carbon monoxide undergoes an isothermal (T = 342 K) volume change from 85 L/mol to 25 L/mol. What is the change in entropy (J/mol-K)?

(d) Gaseous carbon monoxide undergoes a state change from T1 = 342 K and P1 = 4.5 MPa to T2 = 275 K and P2 = 0.13 Mpa? What is the change in entropy (J/mol-K)?

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