A sample of an ideal gas has a volume of 3.55 L 3.55 L at 10.40 ∘ C 10.40 ∘C and 1.30 atm. 1.30 atm. What is the volume of the gas at 21.20 ∘ C 21.20 ∘C and 0.994 atm?

he combined gas law makes use of the relationships shared by pressure, volume, and temperature: the variables found in other gas laws, such as Boyle's law, Charles' law and Gay-Lussac's law.

When we put Boyle's law, Charles' law, and Gay-Lussac's law together, we come up with the combined gas law, which shows that:

Pressure is directly proportional to temperature, or higher temperature equals higher pressure.
Volume is directly proportional to temperature, or higher temperature equals higher volume.
Pressure is inversely proportional to volume, or higher volume equals lower pressure.

expressed mathematically as;

[tex]\frac{PV}{T} = K[/tex]

The formula for the combined gas law can be adjusted to compare two sets of conditions in the same substance.

it is expressed as;

[tex]\frac{P_{1}V_{1} }{T_{1} } = \frac{P_{2}V_{2} }{T_{2} }[/tex]

[tex]P_{1} = 1.30 atm \\P_{2} = 0.99 atm\\V_{1} = 3.55L \\V_{2} = ?\\T_{1} = 10.40^{o} C = 10.40^{o} C + 273^{o} C = 283.4 K\\T_{2} = 21.20^{o}C + 273^{o}C = 294.2 K[/tex]

[tex]V_{2} = \frac{P_{1}V_{1} T_{2} }{T_{1}P_{2} } = \frac{1.30 atm * 3.55 L * 294.2 K}{283.4 K *0.99 atm} = 4.8197 L[/tex]