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12 Dec 2019

Chemical Engineering Question:

An ideal gas with Cp=30 J/mol/K, undergoes the following reversible steps in a closed system:

From T1=300 K, P1=1 bar, to P2=8 bar by adiabatic compression, to P3=1 bar by isothermal expansion, and finally back to the initial state by constant-pressure process. Determine the amount of heat and work in each step of the process and also the total amounts for the entire process.

Summarize your results in a table.

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Trinidad Tremblay
Trinidad TremblayLv2
13 Dec 2019

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Related questions

For the Carnot cycle assuming an ideal gas and reversible processes, determine the change in entropy, dSsys, of the system (not the surroundings) for each of these four steps.

Step 1: isothermal expansion from (V1,P1, T1) to (V2, P2, T1).

Step 2: adiabatic expansion from (V2, P2, T1) to (V3, P3, T2).

Step 3: isothermal compression from (V3, P3, T2) to (V4, P4, T2).

Step 4: adiabatic compression from (V4, P4, T2) to (V1,P1, T1)

Consider a completely reversible cyclic process using the following Carnot cycle with argon gas (behaving ideally) as the working substance:

(A→B) isothermal reversible expansion at 500.0 K from an initial volume of 3.000 L and pressure of 10.00 bar to a final volume of 8.000 L.

(B→C) adiabatic reversible expansion until the temperature falls to 250.0 K.

(C→D) isothermal reversible compression at 250.0 K.

(D→A) adiabatic reversible compression back to the initial conditions.

(a) Using spreadsheets, plot the cycle quantitatively (P vs V). Label each step.

(b) Calculate q, w, ∆U, ∆H, and ΔS for each step and for the overall cycle. Make a table of the results.

(c) Calculate the efficiency of the cycle.

a sample of 1.000 mole of an ideal monatomic gas at 300.0 K and1.00 bar is taken through the following cycle.

a) constant volume heating to twice its initial temperature,followed by

b) reversible adiabatic expansion back to its initial T,followed by

c) reversible isothermal compression back to its initialpressure.

calculate w,q,and delta U (using the ideal gas expression forthe internal energy of a gas) for each of the steps and the overallprocess.

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