Xenon fluoride can be prepared by heating a mixture of Xe and F2 gases to a high temperature in a pressure-proof container.  Assume that xenon gas was added to a 0.25 liter container until its pressure reached 0.12 atm at 0.0°C. Fluorine gas was then added until the total pressure reached 0.72 atm at 0.0°C.  After the reaction was complete, the xenon was consumed completely, and the pressure of the F2 remaining in the container was 0.48 atm at 0.0°C.   What is the empirical formula of the xenon fluoride?

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 200.0°C, the pressure is 1.20 atm, and the mole fraction of O2 in air is 0.210.

Calculate the partial pressure of each component in a mixture of gases contains 3.50 g N2, 2.50 g H2, and 5.27 g of NH3, if the temperature is 25 Celcius and the volume of the mixture is 1.00 L. Please help me solve this one with steps. I thought that it would be the same as calculating with moles, but I'm not even sure anymore.

1. A 5.85 g sample containing only MgO and CuO is placed in a 5.00 L container. The container is filled with CO₂ to a pressure of 740 torr at 20°C. After the reaction has gone to completion, the pressure inside the flask is 290 torr at 20°C. What is the mass percent of MgO in the mixture? Assume that only MgO reacts with CO2.

A sample of an ideal gas at 1.00 atm and a volume of 1.90 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 80.0 atm, what was the volume of the sample? Assume that the temperature was held constant. V = L

For many purposes we can treat ammonia  NH3  as an ideal gas at temperatures above its boiling point of  −33.°C .   Suppose the temperature of a sample of ammonia gas is raised from  −14.0°C  to  −1.0°C , and at the same time the pressure is increased by  15.0% .       Does the volume of the sample increase, decrease, or stay the same?   increase decrease stays the same       If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent. %

A gas mixture contains 2.9 moles of hydrogen, 8.9 moles of carbon dioxide, and 2.7 moles of nitrogen in a 5 L flask. If the total pressure in the flask is 9.35 x 103 mmHg and the partial pressure of carbon dioxide is x atm, what is the value of x?

A certain amount of chlorine gas was placed inside a cylinder with a movable piston at one end. The initial volume was 3.00 LL and the initial pressure of chlorine was 1.25 atmatm . The piston was pushed down to change the volume to 1.00 LL. Calculate the final pressure of the gas if the temperature and number of moles of chlorine remain constant.. (Figure 1) Express your answer with the appropriate units.

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 205.0°C, the pressure is 1.25 atm, and the mole fraction of O2 in air is 0.210.

For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is lowered from 19.0°C⁢ to −17.0°C, and at the same time the pressure is changed. If the initial pressure was 2.2 atm and the volume decreased by 45.0%, what is the final pressure?