Question

A sample of 4.59 L of CO2 gas has a pressure of 7.56 atm. What volume (in Liters) would the gas occupy if the pressure was reduced to 2.57 atm and the temperature raised from 25.0oC to 39.0oC?

Answer 1

The answer to your question is V = 14.44 L

Step-by-step explanation:

Data

Conditions 1 Conditions 2

V1 = 4.69 L V2 = ?

P1 = 7.56 atm P2 = 2.57 atm

T1 = 25°C T2 = 39°C

Process

1.- Convert the temperature to °K

T1 = 25 + 273 = 298°K

T2 = 39 + 273 = 312 °K

2.- Find V2 using the combined gas law

(P1V1)/T1 = (P2V2)/T2

solve for V2

V2 = (P1V1T2) / (T1P2)

substitution

V2 = (7.56 x 4.69 x 312) / (298 x 2.57)

Simplify

V2 = 11062.39 / 765.86

Result

V2 = 14.44 L