The pressure of a gas changes as the volume and temperature of the gas vary. Write a program that uses the Van der Waals equation of state for a gas, (P + (a*n^2) / V^2) * (V - b*n) = n*R*T to display in tabular form the relationship between the pressure and the volume of n moles of carbon dioxide at a constant absolute temperature (T). P is the pressure in atmospheres, and V is the volume in liters. The Van der Waals constants for carbon dioxide are: a = 3.592 (L^2*(atm/mol^2) and b = 0.0427 L/mol. Use 0.08206 (L*atm)/(mol*K) for the gas constant R. Inputs to the program include n, the Kelvin temperature, the initial and final volumes in milliliters, and the volume increment between lines of the table. Your program will output a table that varies the volume of the gas from the initial to the final volume in steps prescribed by the volume increment. Here is a sample run: Please enter at the prompts the number of moles of carbon dioxide, the absolute temperature, the initial volume in milliliters, the final volume, and the increment volume between lines of the table. Quantity of carbon dioxide (moles)> 0.02 Temperature (Kelvin)> 300 Initial volume (milliliters)> 400 Final volume (milliliters)> 600 Volume increment (milliliters)> 50 Output File

0.0200 moles of carbon dioxide at 300 Kelvin Volume (ml) Pressure (atm) 400 1.2246 450 1.0891 500 0.9807 550 0.8918 600 0.8178

Answer rating: 100% (QA)

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