What law deals with temperature and volume?

A gas has a volume of 45 liters at a pressure of 90.8 kPa. If the volume is increased to 55 liters, what will be the new pressure? Round answer to one decimal place.

A gas occupies a volume of 5.6 liters at a temperature of 100 degrees Celsius. To what temperature must the gas be lowered, if it is to occupy 4.0 liters? Answer in Kelvin to one decimal place.

A gas filled weather balloon with a volume of 55.0 liters is released at sea-level conditions of 755 torr. The balloon can expand to a maximum volume of 835 liters. What is the pressure at which this volume is reached? Round answer to one decimal place.

A sample of sulfur hexafluoride gas occupies a volume of 5.10 liters at 198 degrees Celsius. What temperature is needed to reduce the volume to 2.50 liters? Round answer to one decimal place.

Temperature and pressure are ____________ proportional.

If the pressure in a balloon remains constant what happens to the balloon's volume as the temperature of the air increases?

When the volume of air decreases, what happens to pressure?

Each of the flasks shown above have different volumes (they are different sizes) but the temperature of each flask is the same. In which flask will the pressure be the highest?

If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature, what is the new volume?

A gas with a volume of 4.0 L at a pressure of 205 kPa is allowed to expand to a volume of 12.0 L. What is the pressure in the container if the temperature remains constant?

Calculate the new temperature when 6.00 L at 20.0 °C is compressed to 4.00 L.

A container containing 5.00 L of a gas is collected at 100 K and then allowed to expand to 20.0 L. What must the new temperature be in order to maintain the same pressure (as required by Charles' Law)?

A gas at 1580 mm Hg is 389°C. What will the temperature be if the pressure is reduced to 287 mm Hg?

A gas balloon has a volume of 106.0 liters when the temperature is 45.0°C and the pressure is 740.0 mm of mercury. What will its volume be at 20.0°C and 780.0 mm of mercury pressure?

The pressure of a gas is reduced from 1200.0 mm Hg to 850.0 mm Hg as the volume of its container is increased by moving a piston from 85.0 mL to 350.0 mL. What would the final temperature be if the original temperature was 90.0°C?

Avogadro's law states that:

Charles's law states that:

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

Find the volume occupied by 22.0 g of helium gas at 25.0 ^o C and 1.18 atm .

Which of the following term does not involve an ideal gas law ?

Which statement correctly describes a sample of gas in a sealed container?

What Gas Law would you use to solve the following: You have a gas that has a pressure of 2 ATM and a volume of 10L. What would be the new volume if the pressure was changed to 1 ATM?

Determine the temperature, in Kelvin, required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.

A scientist needs to store 28.0 moles of xenon gas at STP in the lab. What size gas tank will he need?

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

A sample of gas containing 8.1 moles at STP would fill a container of what volume?

A water bottle at STP is cooled to -155°C. What is the new pressure?

A student places four gases into a container. The pressures of the gases are: N₂=2.1 atm, H₂=1.3 atm, He=1.9 atm & Ar=3.4 atm. What is the total pressure?

Avogadro's Law explains the relationship between

What is the volume of a balloon that contains 3.7 moles of helium at 75°C and 5.1 atm?

Absolute zero is

What formula would you use to solve the following: A 0.562 L container of Helium has a pressure of 9.5 atm. What volume would be necessary to decrease the pressure to 2.4 atm?

What formula would you use to solve the following: A sample of nitrogen gas was collected over water at a temperature of 23.0°C. What is the partial pressure of nitrogen if the atmospheric pressure (total) was 785 mmHg and the vapor pressure of water was 21.1 mmHg?

What formula would you use to solve the following: A container of carbon monoxide gas is at a temperature of 65.0 °C and occupies a volume of 6.5L. At what temperature would it occupy a volume of 10.2L?

What formula would you use to solve the following problem: A gas at 880mmHg and 298K occupies a container with an initial volume of 1.00 L. The pressure increases to 1980mmHg as the temperature rises to 398K. What will be the new volume?

What formula would you use to solve the following: At high altitudes, pilots have to supplement their supply of oxygen. In this mixture, there are oxygen and nitrogen gases. If nitrogen’s partial pressure is 250mmHg, calculate the partial pressure of oxygen if the total pressure is 710mmHg.

What formula would you use to solve the following: 6.25L of nitrogen gas is known to contain 5.21 moles. If the amount of nitrogen is increased to 12.64 moles, what new volume will result (at unchanged temperature and pressure)?

What formula would you use to solve the following problem: A container has an initial volume of 4.5 L, a pressure of 450 kPa and is at a temperature of 15^oC. If the container is expanded to 6.5 L while the pressure is decreased to 125 kPa, find the resulting temperature.

What formula would you use to solve the following question: How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of

12.4 atm and a temperature of 850 C?

2H₂(g) + O₂(g) --> 2H₂O(l)

What formula would you use to solve the following: If a cylinder has a volume of 5.4 x 106 L of air at a pressure of 140 kPa and it is determined that there are 3.0 x 105 moles of CO2 present, calculate the temperature inside the cylinder.

What formula would you use to solve the following problem: 76 L of compressed oxygen is at a temperature of 330 K. If there are 7.3 moles of oxygen in the container, calculate the pressure (in atm) inside the container.

Which of the following is NOT a unit of Pressure?

In the Question: A cylinder has a volume of 5.4 L of air at a pressure of 140 atm. If the volume is increased to 12.4L, what would the new pressure be? Which answer choice has the data correctly labeled?

What is another way of saying "Number of collisions"?

What is another way of saying "Space"?

What is another way of saying "Speed of particles"?