Question

A sample of gas is at a pressure of 2.81 atm, 664 K, and a volume of 713 L. What will
be the pressure of the gas if its volume and temperature change to 126 L, and 368 K
respectively?

Answer 1

Answer:

8.81 atm

Explanation:

P1 V1 /T1 = P2 V2 / T2              T   must be in Kelvin

re-rrange to :

P1 V1 / T1  *  T2/V2  = P2

2.81 * 713 / (664)  *  368 /126  = 8.81 atm

Answer 2

The new pressure of the gas given that its volume and temperature change to 126 L and 368 K respectively is 8.81 atm

Data obtained from the question

• Initial pressure (P₁) = 2.81 atm
• Initial volume (V₁) = 713 L
• Initial temperature (T₁) = 664 K
• New Volume (V₂) = 126 L
• New temperature (T₂) = 368 K
• New pressure (P₂) = ?

How to determine the new pressure

The new pressure of the gas can be obtained by using the combined gas equation as illustrated below:

P₁V₁ / T₁ = P₂V₂ / T₂

(2.81 × 713) / 664 = (P₂ × 126) / 368

Cross multiply

664 × 126 × P₂ = 2.81 × 713 × 368

Divide both side by 664 × 126

P₂ = (2.81 × 713 × 368) / (664 × 126)

P₂ = 8.81 atm

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