When a certain gas under a pressure of 5.00 * 106 Pa at 25.0°C is allowed to expand to 3.00 times its original volume, its final pressure is 1.07 * 106 Pa. What is its final temperature?

191.316 K or - 81.684 °C

Explanation:

From general gas law,

P₁V₁/T₁ = P₂V₂/T₂ ... Equation 1

Where P₁ = Initial pressure, V₁ = Initial volume, T₁ = Initial temperature, P₂ = Final pressure, V₂ = Final volume, T₂ = Final Temperature.

Make T₂ the subject of the equation.

T₂ = P₂V₂T₁/P₁ V₁ ... Equation 2

Given: P₁ = 5.00*10⁶ Pa, T₁ = 25.0°C = 298 K, P₂ = 1.07*10⁶.

Let: V₁ = y cm³, V₂ = 3y cm³

Substitute into equation 2,

T₂ = (1.07*10⁶*298*3y) / (5.00*10⁶*y)

T₂ = 191.316 K.

Hence the final temperature = 191.316 K or - 81.684 °C