A 1 mol sample of gas has a temperature of 225K, a volume of 3.3L, and a pressure of 500 torr. What would the temperature be if the amount of gas remains constant while pressure dropped to 210 torr, and the volume dropped to 2.75L?

78.75 K

Explanation:

We are given;

Initial pressure, P₁ = 500 torr Initial temperature, T₁ = 225 K Initial volume, V₁ = 3.3 L Final volume, V₂ = 2.75 L Final pressure, P₂ = 210 torr

We are required to calculate the new temperature, T₂

To find the new temperature, T₂ we are going to use the combined gas law; According to the combined gas law;

P₁V₁/T₁ = P₂V₂/T₂

We can calculate the new temperature, T₂;

Rearranging the formula;

T₂ = (P₂V₂T₁) : (P₁V₁)

= (210 torr * 2.75 L * 225 K) : (500 torr * 3.3 L)

= 78.75 K

Therefore, the new volume of the sample is 78.75 K