A cylinder contains 0.250 mole of carbon dioxide gas at a temperature of 27.0°C.

Question

A cylinder contains 0.250 mole of carbon dioxide gas at a temperature of 27.0°C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm (1.013×105 Pa) on the gas. The gas is heated until its temperature increases to 127.0°C. Assume that the CO2 may be treated as an ideal gas. (a) Draw a pV-diagram for this process. (b) How much work is done by the gas in this process? (c) What is the change in internal energy of the gas?

I'm not sure what equations to use. Any help is appreciated!

Answers are below

a) A horizontal line at 1.00 atm from V1 = 6.15×10-3 m3 to V2 = 8.20×10-3 m3.

b) 208 J.

c) 312 J.

Explanation / Answer

a)    Here,   a pV-diagram for this process is :-

   A horizontal line at 1.00 atm from V1 = 6.15×10-3 m3 to V2 = 8.20×10-3 m3.

b)    work is done by the gas in this process = P * (V2 - V1)

                                                     = 1.013 * 105 * (8.20×10-3 - 6.15×10-3)

                                                      = 208 J

c)    the change in internal energy of the gas   = 3/2 * n * R * T

                                                                         = 3/2 * 0.250 * 8.314 * 100

                                                                        = 312 J

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