A sample of a gas mixture contains the following quantities of three gases. compound mass CO 1.72 g CO2 3.36 g SF6 3.52 g The sample has: volume = 2.50 L temperature = 16.6 °C What is the partial pressure for each gas, in mmHg? What is the total pressure in the flask? CO 0.59 x mmHg CO2 0.73 x mmHg SF6 23.21 X mmHg total 24.54 x mmHg

A 22.4 L sample of a gas is heated from 15 °C to 78 °C. What volume (mL) does the gas occupy at the higher temperature if the pressure remains constant? O 2.7 x 104 mL O 27 mL O 1.8 x 10 mL 1.2 x 105 mL

The volume of a sample of hydrogen gas was decreased from 12.14 L to 5.43 L at constant temperature. If the final pressure exerted by the hydrogen gas sample was 9.75 atm, what pressure did the hydrogen gas exert before its volume was decreased? P = atm

A mixture of nitrogen, oxygen and argon has a total pressure of 728 mmHg. The partial pressures of oxygen and argon are 234 mmHg and 135 mmHg respectively. What is the partial pressure of nitrogen?

The initial volume of an ideal gas is 3.0 L. If the pressure triples at constant temperature and constant moles, what is the final volume? 6.0 L 3.0 L   1.0 L

A quantity of N2 gas originally held at 5.25 atm in a 1.00 L container at 26 °C is transferred to a 12.5 L container at 20 °C. A quantity of O, originally at 5.25 atm and 26 °C in a 5.00 L container is transferred to the same container. What is the total pressure of the mixture in the new container?

Consider the apparatus shown below with the valve closed. The volume and pressure of each gas is indicated. F2 N2 Valve 3.00 L 6.00 L 2.00 atm 4.00 atm When the valve is opened the two gases mix uniformly. At that point, what is the mole fraction of nitrogen in the mixture? 0.800 none of the answers are correct 0.500 0.333