Question

A 35.0 L sample of gas collected in the upper atmosphere at a pressure of 48.6 torr is compressed into a 150. mL container at constant temperature. What is the new pressure (atm)? (4pts) 1 atm = 760 torr

Answer 1

The new pressure (atm) = 14.7 atm or 11172 torr

Step-by-step explanation:

P₁V₁ = P₂V₂ (using Boyle's law at constant temperature)

Volume of sample of gas collected in the upper atmosphere (V₁) = 35.0 Lit

pressure of the gas (P₁) = 48.6 torr

1 atm = 760 torr

⇒
`1 torr= (1)/(760) = 0.00131 atm`

⇒ 48.6 torr = 48.6 x 0.00131 = 0.063 atm

Volume after compression (V₂) = 150 ml = 0.15 lit

New pressure (P₂) = ?

P₁V₁ = P₂V₂

⇒ P₂ =
`(P_(1) V_(1) )/(V_(2) ) \\`

⇒ P₂ =
`=(0.063X35)/(0.15) = 14.7 atm` or 11172 torr