Question

The pressure of a gas is reduced from 1200 torr to 760 torr as the volume of its container is increased from 0.650 L to 1.1 L. What would the final temperature be in Celsius if the original temperature was 15 C?

Answer 1

-272.99K = 0.0032°C

Step-by-step explanation:

Applying (P1V1)/T1 = (P2V2)/T2

(1200×0.65)/288 = (760 × 1.1)/T2

Simplify

T2 = 0.0032°C

Answer 2

The final temperature would be 308.7 K or 35.7 °C

Step-by-step explanation:

Step 1: Data given

The initial pressure = 1200 torr

The pressure is reduced to 760 torr

The initial volume = 0.650 L

The increased volume is 1.1 L

The initial temperature is 15 °C = 288 K

Step 2: Calculate the new temperature

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

⇒with P1 = the initial pressure = 1200 torr

⇒with V1 = the initial volume = 0.650 L

⇒with T1 = initial temperature is 15 °C = 288 K

⇒with P2 = the reduced pressure = 760 torr

⇒with V2 = the increased volume = 1.1 L

⇒with T2 = the final temperature = TO BE DETERMINED

(1200 torr * 0.650 L) / 288 K = (760 torr * 1.1 L) / T2

T2 = (760 * 1.1 * 288) / (1200 * 0.650)

T2 = 308.7 K

The final temperature would be 308.7 K or 35.7 °C