A graduate student wants to use van der Waals' equation to express the pressure-volume- temperature relations for a gas. Her project requires a reasonable degree of precision in the p-V-T calculations. Therefore, she made the following experimental measurements with her setup to get an idea of how easy the experiment would be: Temperature, K Pressure, atm Volume, ft/lb mol 1.860 200 0.741 273.1 273.1 1000 Determine values of constants a and b to be used in van der Waals' equation that best fit the experimental data.

Liquid nitrogen has a density of 0.808 g/mL and boils at 77 K. Researchers often purchase liquid nitrogen in insulated 175-L tanks. The liquid vaporizes quickly to gaseous nitrogen (which has a density of 1.15 g/L at room temperature and atmospheric pressure) when the liquid is removed from the tank. Suppose that all 175 L of liquid nitrogen in a tank accidentally vaporized in a lab that measured 10.00m x 10.00m x 2.50m. What maximum fraction of the air in the room could be displaced by the gaseous nitrogen?

A 370-g sample of an unknown (nongaseous) material experiences a 24.0°C increase in temperature after absorbing 1.24 x 103) of energy. (a) What is the specific heat of this material? 3400 Your response differs significantly from the correct answer. Rework your solution from the beginning and check each step carefully. J/(kg. °C)