A rigid, metal container of oxygen gas holds 55 L of gas. It has a pressure of 4.6 atm at a temperature of 545 K. What is the new pressure of standard temperature, 0°C?

A rigid, sealed container that can hold 23 L of gas is filled to a pressure of 6.56 atm at 361 °C. The pressure suddenly decreases to 4.60 atm. What is the new temperature inside the container, in units of °C? Do not include units in your answer.

Three identical balloons (shown below) are filled to the same volume. Temperature and pressure are kept constant (25°C and 101.3 kPa, respectively). Which balloon contains the smallest mass of gas? Explain your reasoning.

2a

A sample of xenon gas occupies 71.1 litres under a pressure of 1.55 x 103 torr at 25.0 °C. What volume (in litres) would this sample occupy at -72.8 °C, if the pressure remained constant? Assume xenon acts as an ideal gas. Enter the numerical value (no units), using 3 significant figures. Type your answer...

A.) What is the temperature of 0.45 mol of gas at a pressure of 1.0 atm and a volume of 12.0 L ? Express the temperature in kelvins to two significant figures.   B.) A weather balloon is inflated to a volume of 25.9 L at a pressure of 752 mmHg and a temperature of 27.5∘C. The balloon rises in the atmosphere to an altitude where the pressure is 400. mmHg and the temperature is -15.3∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

A colleague of yours takes a bunch of pressure readings while you are gone. You return to realize that he has invented a new unit: his body mass of 180lb per 1mile?. He calls this unit Bob per Bob's Block. 1mile = 63360 inches. What is the pressure of 9 Bobs per Bob's block in a real unit of pressure, pounds per square inch (PSI)? Use just one sig fig in your answer: x10^ PSI

A helium-filled weather balloon has a volume of 506 L at 19.9°C and 758 mmHg. It is released and rises to an altitude of 5.40 km, where the pressure is 462 mmHg and the temperature is –14.1°C. The volume of the balloon at this altitude is ___ L.

Dinitrogen monoxide gas is collected at −4.0°Cin an evacuated flask with a measured volume of  50.0L. When all the gas has been collected, the pressure in the flask is measured to be 0.360atm. Calculate the mass and number of moles of dinitrogen monoxide gas that were collected. Be sure your answer has the correct number of significant digits.

Calculate the final pressure of the gas. Round your answer to  3 significant digits.