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19 Nov 2019

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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Jarrod Robel
Jarrod RobelLv2
29 May 2019

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cyclic process

Consider an ideal gas with molar constant volume heat capacity, cV,m = 1.50 R. The gas undergoes the reversible four step cyclic process shown to the left: 1. During step 1, the gas expands isothermally from V1 to V2. 2. During step 2, the gas expands adiabatically from V2 to V3. 3. During step 3, the gas is compressed isothermally from V3 to V4. 4. During step 4, the gas is compressed adiabatically from V4 to V1. Given T1 = 350.0 K, P1 = 1.00 × 105 Pa, V1 = 5.82 × 10-2 m3 , V2 = 10.0 × 10-2 m3 , T3 = 175.0 K,

Perform the following calculations:

a. Determine the pressure, volume, and temperature of the gas at equilibrium points 1, 2, 3, and 4.

b. Calculate the work done on the gas during each step.

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d. Calculate the change in energy of the gas during each step.

e. Calculate q, w, and ΔU for the entire cyclic process.

f. Determine the enthalpy of the gas at equilibrium points 1, 2, 3, and 4.

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DearChegg Lifesaver. Here are the requirements:

1.Use given values as stated in questions below.

2.Clearly State Answer

3.(Please) LEAVE A COMMENT if you are currently working on anyproblems.

4.Formany of these problems you will need to use tabulated thermodynamicdata. Use the Information provided after problem 17.



---------------------------------------Questions---------------------------------------------------



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SiO2(s)+ 4HF(g) ? SiF4(g) + 2H2O(g)


3.Use heat of formation data to determine ?H° for the reaction:

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4.Calculate the mass of methane that must be burned to provide enoughheat to convert 330.0 g of water at 37.0°C into steam at 124.0°C.(Assume that the H2Oproduced in the combustion reaction is steam rather than liquidwater.)


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C2H2(g)+ 5/2 O2(g) ? 2 CO2(g) + H2O(g)

with?H° = -1255.8 kJ.

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6.Given the following data:

HNO3(l)? 1/2N2(g) + 3/2O2(g) + 1/2H2(g) ?H° = 174.1 kJ

2N2O5(g)? 2N2(g) + 5O2(g) ?H° = -28.4 kJ

H2O(l)? H2(g) + 1/2O2(g) ?H° = 285.8 kJ


Calculate?H° for the reaction:

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C2H4(g)+ Cl2(g) ? CH2ClCH2Cl(g)



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Allsystems become more disordered spontaneously.

Both?Ssys and ?Ssurr must equal zero at equilibrium.

Theentropy of the universe is constant; the energy of the universedecreases towards a minimum.

Allspontaneous processes release heat.

Ifa reaction is spontaneous, the reverse reaction is non-spontaneous.

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