A chemist has a certain amount of gas under a pressure of 33.3 atm; it occupies 30.0 L at 273 ◦C. For his research, however, the gas must be at STP. What will the volume if the gas be?

Question

Chemistry

Cullen Riley

5 February, 16:59

A chemist has a certain amount of gas under a pressure of 33.3 atm; it occupies 30.0 L at 273 ◦C. For his research, however, the gas must be at STP. What will the volume if the gas be?

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Answers (1)

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Jada Johnson · Answer 1

499.5 L

Explanation:

Step 1:

Data obtained from the question. This includes the following:

Initial pressure (P1) = 33.3 atm

Initial volume (V1) = 30L

Initial temperature (T1) = 273°C = 273°C + 273 = 546K

Final pressure (P2) = stp = 1 atm

Final temperature (T2) = stp = 273K

Final volume (V2) = ... ?

Step 2:

Determination of the final volume.

This can be done by using the general gas equation formula as shown below:

P1V1/T1 = P2V2/T2

33.3 x 30/546 = 1 x V2 / 273

Cross multiply to express in linear form

546 x V2 = 33.3 x 30 x 273

Divide both side by 546

V2 = (33.3 x 30 x 273) / 546

V2 = 499.5 L

Therefore the volume of the gas will be 499.5 L