A glass container was initially charged with 1.80 moles of a gas sample at 4.25 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 30.1 °C, so the final pressure in the container was reduced to 1.25 atm. How many moles of the gas sample are present at the end?

An ideal gas is contained in a cylinder with a volume of 5.1*10^2 mL at a temperature of 30.°C and a pressure of 710. torr. The gas is then compressed to a volume of 27 mL, and the temperature is raised to 820.°C. What is the new pressure of the gas? Pressure =  torr

A sample of an ideal gas at 1.00 atm and a volume of 1.64 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 30.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

A glass container was initially charged with 2.35 moles of a gas sample at 3.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 28.1 °C, so the final pressure in the container was reduced to 0.998 atm. How many moles of the gas sample are present at the end?

A sample of xenon gas occupies a volume of 7.22 L at 52.0°C and 0.710 atm. If it is desired to increase the volume of the gas sample to 8.89 L, while increasing its pressure to 0.963 atm, the temperature of the gas sample at the new volume and pressure must be °C.

Hydrogen gas, H₂, and oxygen gas, O₂, can be reacted to form liquid water. If 2.00 g hydrogen gas and17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in theflask at 25 °C. The vapor pressure of water is 32.8 mm Hg. Stoichiometry is involved in this question.Total gas pressure:

Container A holds 752 mL of ideal gas at 2.30 atm. Container B holds 124mL of ideal gas at 4.70 atm. If the gases are allowed to mix together, what is the partial pressure of each gas in the total volume?

For many purposes we can treat ammonia (NH, ) 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 13.0 °C to –16.0 °C, and at the same time the pressure is increased by 10.0%. increase x10 Does the volume of the sample increase, decrease, or stay the same? 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.

4. A glass container was initially charged with 2.00 moles of a gas sample at 3.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 28.1 °C, so the final pressure in the container was reduced to 0.998 atm. Assume the volume stayed the same. How many moles of the gas sample are present at the end?