1. How many atm of gas did you add to the flask? A. 1 atm B. 3 atm C. 4 atm D. 2 atm 2. What was the volume of the flask? E. 100 mL F. 120 mL G. 150 mL H. 88 mL 3. How many grams of propane were there in 1 atm? Choose the closest answer. I. 0.735 g J. 0.274 g K. 0.664 g L. 0.232 g 4. How many grams of butane were there in 1 atm of gas? Choose the closest answer. M. 0.774 g N. 0.361 g O. 0.664 g P. 0.214 g 5. How many grams of methane were in 1 atm of gas? Choose the closest answer. Q. 0.244 g R. 0.337 g…show more content… Which of the following relationships best describes the results of your experiment? P = pressure, V=volume, n=number of moles, R=gas constant, T=temperature, and C=a constant u. V/n=C v. R/T=C w. T/n=C x. P/n=C 15. In a real gas (non-ideal), the molecules can interact with each other. Suppose that the primary interaction between the molecules is attractive. How would this affect the results? y. The pressure would be higher for a more strongly attracting gas. z. There would be no difference. {. The pressure becomes independent of the identity of the molecules. |. The pressure would be lower for a more strongly attracting gas. 16. Suppose you had a mixture of gasses. Which of the following is false? }. The pressure of the gas is equal to the sum of the partial pressures of the constituent gases. ~. The pressure of the gas depends on the identity of the molecules in the gas. . The gas will behave as an ideal gas to a first approximation. . The gas will expand to fill its container. 17. In an ideal gas, P*V = n*R*T where P = pressure, V=volume, n=number of moles, R=gas constant, and T=temperature. Consider a gas with pressure = 1 atm, 1 mole of molecules, and a temperature of 295 K. R=0.082 atm*L/(mol * K). How much volume should this gas occupy? Choose the closest answer. . 1.0 L . 22.4 L . 30.6 L .
