If a sample of a gas is initially at 755 mmHg 12.6L and 22.4 C what will be the new pressure if the volume is reduced by 2.5 L and the temperature is 33.3 C

Answer 1

To solve this problem, we can use the combined gas law formula:

P₁V₁/T₁ = P₂V₂/T₂

Where:
P₁ = initial pressure (755 mmHg)
V₁ = initial volume (12.6 L)
T₁ = initial temperature in Kelvin (22.4 °C + 273.15 = 295.55 K)
P₂ = unknown final pressure
V₂ = final volume (12.6 L - 2.5 L = 10.1 L)
T₂ = final temperature in Kelvin (33.3 °C + 273.15 = 306.45 K)

Plugging the given values into the formula, we get:

(755 mmHg)(12.6 L)/(295.55 K) = P₂(10.1 L)/(306.45 K)

Simplifying the equation, we have:

P₂ = (755 mmHg)(12.6 L)(306.45 K)/(295.55 K)(10.1 L)

P₂ ≈ 987 mmHg

Therefore, the new pressure of the gas, when the volume is reduced by 2.5 L and the temperature is increased to 33.3 °C, is approximately 987 mmHg.