Question

The pressure on 7.0 L of gas is increased from 15 psi to 1420 torr, at constant

temperature. What is the new volume of the gas?​

Answer 1

3.85L

Step-by-step explanation:

Given parameters:

Initial pressure P₁ = 15psi (1psi = 52mmHg)

converting to mmHg gives (15x52)mmHg = 780mmHg

Initial volume V₁ = 7.0L

Final pressure P₂ = 1420torr= 1420mmHg

Unknown:

Final volume V₂ = ?

Condition of the process: Constant temperature

Solution

To solve this problem, we simply apply Boyle's law. Boyle's law states that "The volume of a given mass of gas varies inversely as the pressure changes, if the temperature is constant".

It is mathematically expressed as ;

P₁V₁ = P₂V₂

The unknown here is V₂ and we simply express it as the subject of the formula:

V₂ =
`(P_(1) V_(1) )/(P_(2) )`

V₂ =
`(780 x 7 )/(1420)`

V₂ =
`(5460)/(1420)` = 3.85L