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?

Question

Chemistry

Lyric Wallace

24 September, 04:50

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?

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Answers (1)

Know the Answer?

Valentino Fitzpatrick · Answer 1

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