A 1.0 L volume of gas at 760 mm Hg and 25 degrees celsius is transfered to a 0.8 L container at 5 degrees celc

You need to use the ideal gas law to answer this question

(P1 * V1)/T1 = (P2 * V2)/T2

T is in Kelvins so you must convert from degrees celsius to Kelvin, so your temeprastures are T1 = 298 K, T2 =278 K

So (760 mmHg * 1.0 L)/298 K = (P2 * 0.8 L)/278 K

(760 mmHg * 1.0 L * 278K)/(0.8 L * 298 K) = P2

P2 = 886 mmHg

just by looking at the problem you can eliminate C because increasing the temperature would increase the volume when the pressure is constant. to find the answer you would plug the data into the V1/T1=V2/T2 25 degrees C =298K 100degree C = 373K 5.00L / 298K = V2 / 373K V2= 5.00L x 373 K / 298K V2= 6.26 L so D would be the correct answer

I believe in this question, your moles are constant.

Use the formula:

p1v1/T1 = p2v2/T2

p1 = 760mmHg

v1= 1.0-L

v2 = 0.8-L

T1 = 25 degrees = 298.15 Kelvins

T2 = 5 degrees = 278.15 Kelvins

p2 = ?

p2 = p1v1T2/v2T1

= (760mmHg)(1.0-L)(278.15K)/(0.8-L)(298.15K)

= The answer should be 886mmHg

P1*V1/T1=P2*V2/T2

P2=P1*V1*T2/T1/V2

=760(5)/25/.8

=886 mm Hg

my bad, read it as 8.00 at first