7. Gases

Which of the following statements about substances X and Y is true, assuming both behave as ideal gases under identical conditions?

Which of the following laws is directly related to the formulation of the ideal gas law?

Which of the following gas laws can be combined to derive the ideal gas law equation?

A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the balloon contain at 1.35 atm and 253 K, assuming ideal gas behavior?

A sample of hydrogen gas (H2) has a volume of 8.56 L at a temperature of 0 degrees C and a pressure of 1.5 atm. Using the Ideal Gas Law, calculate the moles of H2 molecules present in this gas sample.

Binary compounds of alkali metals and hydrogen react with water to produce H₂(g). The H₂ from the reaction of a sample of NaH with an excess of water fills a volume of 0.510 L above the water. The temperature of the gas is 35°C and the total pressure is 0.980 atm. Using the Ideal Gas Law, what is the number of moles of H₂ produced?

What is the mass of 8.55 L of phosphine gas (PH_3) at STP? Round your answer to 3 significant figures.

A student collects a gas over water using a eudiometer. The atmospheric pressure is 1.00 atm, and the height difference between the water levels inside and outside the eudiometer is negligible. What is the pressure of the collected gas (pgas)?

What happens to the pressure of a gas sample when the volume is halved and its Kelvin temperature is doubled, assuming the amount of gas remains constant?

A balloon is filled with 1.5 moles of helium at room temperature, 25℃, and has a volume of 2.4 L. Calculate the volume of the balloon when it is placed into liquid nitrogen at −196℃. Assume that the pressure remains constant.

What is the volume of 1.00 mole of an ideal gas at 1.00 atm pressure and 0°C?

A 1.20 L weather balloon on the ground has a temperature of 25.0 °C and is at atmospheric pressure (1.00 atm). When it rises to an elevation where the pressure is 0.710 atm, the new volume is 1.80 L. What is the temperature (in °C) of the air at the elevation where the balloon rises?

A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K?

In a chemical reaction involving the decomposition of calcium carbonate (CaCO3), which gas is produced?