XeF₄ is a gaseous compound that only contains fluorine and xenon. A 100.0 mL steel vessel filled with 0.283 g of XeF₄ has a pressure of 0.178 atm at 0 °C. XeF₄ breaks down into its component parts when the vessel is heated up to 117 °C. What are the partial pressures of xenon and fluorine in the container, as well as the total pressure?

The density of a group 2A metal is 1.55 g/cm³ and crystallizes in a cubic unit cell that has an edge length of 653 pm. When a 1.65 cm³ slab of this metal reacts with excess hydrobromic acid, the gas produced occupies a volume of 1.50 L with a pressure of 794 mmHg at 27.0°C. What is the identity of the metal?

A 1.50 L reaction flask contains 14.22% O₂, 61.27% CO₂, and 24.51% water vapor at 30.0°C. The total pressure inside the flask is 24.61 kPa. Calculate the mass of naphthalene (C₁₀H₈) that was burned in order to produce this amount of water vapor. 

C₁₀H₈(s) + 12 O₂(g) → 10 CO₂(g) + 4 H₂O(g)

Consider the following reaction:

Cl₂(g) + F₂(g) → ClF₃(g)     [unbalanced]

At 301 K, a 2.50-L reaction chamber is initially composed of chlorine gas and fluorine gas with a partial pressure of 472 mmHg and 862 mmHg, respectively. Determine the limiting reagent. What is the theoretical yield of ClF₃?

Consider the following reaction:

2 SO₂(g) + O₂(g) → 2 SO₃(g)

At 345 K and 75.0 mmHg, 265.3 mL of SO₃ were collected when 305.2 mL of SO₂ and 176.4 mL of O₂ reacted. What is the percent yield of the reaction?

The following reaction produces 2.50 g of solid potassium chloride. Calculate the total volume of oxygen gas that can be collected over water at 25.0 °C and 760 mmHg. Note that the vapor pressure of water at 25.0 °C is 3.169 kPa.

2 KClO₃ (s) → 2 KCl (s) + 3 O₂ (g)

The hydrogen gas produced from a chemical reaction was collected over water at 40°C with a total pressure of 715 mmHg. (Water pressure is 55.3 mmHg at 40°C.)

a. What would be the partial pressure of the hydrogen gas collected? 

b. What is the mass of hydrogen gas collected if the total volume of gas collected is 763 mL?