Question

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.

Answer 1

2.32

Step-by-step explanation:

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:

`(P)/(T) = Constant` ⇒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:

`(P1)/(T1) = (P2)/(T2)`

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

`P2=(P1 . T2)/(T1)`

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

`P2 = (1.50 atm . 423.15K)/(273.15 K) = 2.3237atm` ≅ 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