A sample of nitrogen gas in a 1.59-L container exerts a pressure of 1.47 atm at 26 ∘C. What is the pressure if the volume of the container is maintained constant and the temperature is raised to 371 ∘C?

New pressure is 3.16 atm

Explanation:

Let's apply the Gay Lussac law for this which states the pressure of a fixed volume of a gas is directly proportional to its temperature.

As the T° raises, the pressure raises too.

Is the T° decreases, the pressure will decrease too.

P₁ / T₁ = P₂ / T₂

First of all, let's convert the T° to aboslute values:

26°C + 273 = 299 K

371°C + 273 = 644 K

1.47 atm / 299 K = P₂ / 644 K

(1.47 atm / 299 K). 644 K = P₂

P₂ = 3.16 atm