7. Gases

In calculations involving the ideal gas law, when must temperature values be expressed in kelvin units?

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112°C. What is the final volume of the gas, in milliliters, when the pressure is changed to 0.85 atm and the temperature is changed to 25°C, assuming the amount of gas remains constant?

Under which of the following conditions does the molar volume of a gas decrease according to the ideal gas law?

If 50.75 g of a gas occupies 10.0 L at STP, how many liters will 129.3 g of the same gas occupy at STP?

Which of the following is NOT a variable in the ideal gas law equation PV = nRT?

Which statement can best be concluded from the ideal gas law?

Which of the following is a common unit for the ideal gas constant R in the Ideal Gas Law?

Based on the behavior of molecules in a mixture of gases, which statement best explains why the ideal gas law (PV = nRT) can be applied to mixtures?

Using the ideal gas law, what is the volume (in liters) occupied by 0.200 mol of an ideal gas at a pressure of 200. kPa and a temperature of 400. K? (Use R = 8.314 L·kPa·mol^{-1}·K^{-1})

A syringe contains 0.65 moles of He gas that occupy 900.0 mL. What volume (in L) will the syringe hold if 0.35 moles of Ne are added, assuming ideal gas behavior and constant temperature and pressure?

Why is it important to convert temperature to units of kelvin before using the ideal gas law?

Which of the following conditions does NOT contribute to greater gas ideality?

Which statement best describes Boyle's Law?

Which gas is primarily transported through the blood as bicarbonate ions?

Why does a sealed bag of chips expand when you take it to a higher altitude?