A 12.0 L sample of argon gas has a pressure of 28.0 atm. What volume would this gas occupy at 9.70 atm?

2 Answers
Jun 6, 2016

The volume that this gas occupies is 34.6 L

Explanation:

Let's start off with identifying our known and unknown variables.
The first volume we have is 12.0 L, the first pressure is 28.0 atm, and the second pressure is 9.70 atm. Our only unknown is the second volume.

We can obtain the answer using Boyle's Law which shows that there is an inverse relationship between pressure and volume as long as the temperature and number of moles remain constant.

The equation we use is P_1V_1=P_2V_2
where the numbers 1 and 2 represent the first and second conditions. All we have to do is rearrange the equation to solve for the volume.

We do this by dividing both sides by P_2 in order to get V_2 by itself like so:
P_1V_1 -:P_2 = V_2

Now all we do is plug and chug!
(28.0 cancel (atm)) (12.0 L) -: (9.70 cancel (atm)) = 34.6 L

Boyle's Law Practice Problems

Jun 6, 2016

V_2-=34.6 L

Explanation:

Use the combined gas low equation.

(P_1xxV_1)/T_1=(P_2xxV_2)/T_2

T_1=T_2 since the temperature remains constant.

P_1xxV_1=P_2xxV_2

V_2=(P_1xxV_1)/P_2

V_2=(28.0\ atm xx 12.0\ L)/(9.70\ atm)

V_2-=34.6 L