Question

X Check significant figures and critical properties. You may wish to experiment with the compressibility charts a bit to make sure that you understand them. For example, you might check consistency of Pr,Tr , and Vr. A volume of 1.4 L of ethylene vapor at −32.5°C and 9.6 atm is heated at constant volume until it reaches a temperature of 179.8°C. Jse the theory of corresponding states and the appropriate compressibility-factor chart to estimate the final pressure of the volume of ethylene. atm

Answer 1

To estimate the final pressure of the volume of ethylene, we can use the theory of corresponding states and the compressibility-factor chart. Here's a step-by-step approach to solving this problem:

1. Identify the given information:

- Initial volume (Vi) = 1.4 L

- Initial temperature = -32.5°C

- Initial pressure (Pi) = 9.6 atm

- Final temperature = 179.8°C

2. Convert the initial and final temperatures to Kelvin:

- Initial temperature = -32.5 + 273.15 = 240.65 K

- Final temperature = 179.8 + 273.15 = 452.95 K

3. Calculate the initial reduced temperature (Tr):

- Tr = Ti / critical temperature (Tc)

- Refer to the compressibility-factor chart to find the critical temperature of ethylene.

4. Calculate the initial reduced pressure (Pr):

- Pr = Pi / critical pressure (Pc)

- Refer to the compressibility-factor chart to find the critical pressure of ethylene.

5. Calculate the initial reduced volume (Vr):

- Vr = Vi / critical volume (Vc)

- Refer to the compressibility-factor chart to find the critical volume of ethylene.

6. Use the compressibility-factor chart to determine the compressibility factor (Z) at the initial reduced conditions (Pr, Tr, Vr).

7. Use the compressibility factor (Z) to estimate the final pressure :

- Pf = Z * critical pressure (Pc)

Make sure to use the appropriate units for each calculation and refer to the compressibility-factor chart specific to ethylene. This approach helps estimate the final pressure based on the given information and the properties of the substance.

Step-by-step explanation: