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?

The answer to your question is V = 14.44 L

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

14 days is the half-life of phosphorus-32

the answer to your question is c