What relationship does Gay-Lussac’s law express?

A 1.0 L volume of gas at $27.0^{\circ} \mathrm{C}$ exerts a pressure of 85.5 kPa. What will the pressure be at $127^{\circ} \mathrm{C}$? Assume constant volume.

How many grams of oxygen gas must be in a 10.0 L container to exert a pressure of 97.0 kPa at a temperature of $25^{\circ} \mathrm{C}$?

How many moles of argon are there in 20.0 L, at $25^{\circ} \mathrm{C}$ and 96.8 kPa?

Solid LiOH can be used in spacecraft to remove $CO_2$ from the air. $2 \mathrm{LiOH}(s)+\mathrm{CO}_{2}(g) \rightarrow \mathrm{Li}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)$ What mass of LiOH must be used to absorb the carbon dioxide that exerts a partial pressure of 5.0 kPa at $15^{\circ} \mathrm{C}$ in a spacecraft with volume of $8.0 \times 10^{4} \mathrm{L}$?

Hot air balloonists use large fans to force air into their balloons. When the balloon is about three quarters full, they turn off the fan and heat the air inside the balloon using a propane burner. As the air is heated, the balloon rises. Once airborne, the balloonist can turn off the burner and just use it occasionally to keep the balloon aloft. The heating of the air in the balloon is a practical application of the gas laws. If the volume of the balloon is 3 000 cubic meters $(m^3)$ at $27^{\circ} \mathrm{C}$, what is its volume at $52^{\circ} \mathrm{C}$, assuming a constant pressure? F. $2750 \mathrm{m}^{3}$, G. $3250 \mathrm{m}^{3}$, H. $4500 \mathrm{m}^{3}$, I. $6250 \mathrm{m}^{3}$.

How many grams of carbon dioxide are contained in 1.000 L of the gas, at $25.0^{\circ} \mathrm{C}$ and 101.325 kPa? What is the density of the gas at these conditions? What would the density of oxygen be at these conditions?

How many liters of hydrogen are obtained from the reaction of 4.00 g calcium with excess water, at $37^{\circ} \mathrm{C}$ and 0.962 atm?

What volume of oxygen, measured at $27^{\circ} \mathrm{C}$ and 101.325 kPa, is needed for the combustion of 1.11 kg of coal? (Assume coal is 100% carbon.) $\mathrm{C}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)$

Suppose a certain automobile engine has a cylinder with a volume of 500.0 mL that is filled with air (21% oxygen) at a temperature of $55^{\circ} \mathrm{C}$ and a pressure of 101.0 kPa. What mass of octane must be injected to react with all of the oxygen in the cylinder? $2 \mathrm{C}_{8} \mathrm{H}_{18}(l)+25 \mathrm{O}_{2}(g) \longrightarrow 16 \mathrm{CO}_{2}(g)+18 \mathrm{H}_{2} \mathrm{O}(g)$

Magnesium will burn in oxygen to form magnesium oxide as represented by the following equation. $2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{MgO}(s)$ What mass of magnesium will react with 500.0 mL of oxygen at $150.0^{\circ} \mathrm{C}$ and 70.0 kPa?

How many liters of hydrogen gas can be produced at 300.0 K and 104 kPa if 20.0 g of sodium metal is reacted with water according to the following equation? $2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g)$

In gas stoichiometry problems, what is the “bridge” between amount in moles and volume?

Why does carbon dioxide gas, which has a sublimation point of $-79^{\circ} \mathrm{C}$, cool enough to become solid as it leaves a fire extinguisher at room temperature?