Consider the following balanced equation in which gas X forms gas $\mathrm {X} _ { 2 } :$ 2$\mathrm { X } ( g ) \longrightarrow \mathrm { X } _ { 2 } ( g )$ Equal moles of X are placed in two separate containers. One container is rigid, so the volume cannot change; the other container is flexible, so the volume changes to keep the internal pressure equal to the external pressure. The above reaction is run in each container. What happens to the pressure and density of the gas inside each container as reactants are converted to products?

Use the postulates of the kinetic molecular theory (KMT) to explain why Boyle's law, Charles's law, Avogadro's law, and Dalton's law of partial pressures hold true for ideal gases. Use the KMT to explain the P versus n (at constant V and T) relationship and the P versus T (at constant V and n) relationship.

Rationalize the following observations. a. Aerosol cans will explode if heated. b. You can drink through a soda straw. c. A thin-walled can will collapse when the air inside is removed by a vacuum pump. d. Manufacturers produce different types of tennis balls for high and low elevations.

Convert the following into balanced equations: (a) When gallium metal is heated in oxygen gas, it melts and forms solid gallium(lll) oxide. (b) Liquid hexane burns in oxygen gas to form carbon dioxide gas and water vapor. (c) When solutions of calcium chloride and sodium phosphate are mixed, solid calcium phosphate forms and sodium chloride remains in solution.

At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of

$$22^\circ C$$

and a pressure of 734 torr. Calculate the mass percent of

$$NaCIO_3$$

in the original sample. (At

$$22^\circ C$$

the vapor pressure of water is 19.8 torr.)