A sample of hydrogen gas at 1.50 atm and constant volume is heated from 0∘C to 150∘C. What will be the final pressure of the gas in atmospheres?
Use −273.15∘C for absolute zero.
Your answer should have three significant figures (round your answer to two decimal places).
Do not include units in your response.

For the resolution of the problem one of the laws of Charles - Gay Lussac must be used, in which it is stated that if a certain amount of gas is kept at a constant volume (as in this case), its pressure will be directly proportional to its absolute temperature. Mathematically, it can be written as follows:

[tex]\frac{P}{T} = Constant[/tex] ⇒to constant V

In the case of the statement, that we have an initial system (P₁ and T₁) and an final system (P₂ and T₂), the equation can be written:

[tex]\frac{P1}{T1} = \frac{P2}{T2}[/tex]

It can be rearranged to clear P₂ which is what needs to be calculated, then:

[tex]P2=\frac{P1 . T2}{T1}[/tex]

It would only be necessary to convert the temperature units from ° C to K, to have the absolute temperature values. If T (K) = t (° C) + 273.15, then:

T₁ = 0 + 273.15 = 273.15 K

T₂ = 150 + 273.15 = 423.15 K

Now, you can replace the values to the equation and calculate P₂

[tex]P2 = \frac{1.50 atm . 423.15K}{273.15 K} = 2.3237atm[/tex] ≅ 2.32 atm

As the statement requests the result with three significant figures and no units, the answer is that the final pressure is 2.32