Question

The pressure of a gas is released from 12.4 atm to 7.1 atm as the volume of its container is decreased by moving each position from 250 ml to 125 ml. What would the final temperature be if the original temperature was 363 K?

a. 726 K
b. 484 K
c. 363 K
d. 242 K

Answer 1

To calculate the final temperature of the gas, we can use the combined gas law equation. Plugging in the given values and solving for the final temperature, we find that the final temperature would be 484 K. Hence, option (b) is correct.

Step-by-step explanation:

To calculate the final temperature of the gas, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

Where:

• P1 is the initial pressure
• V1 is the initial volume
• T1 is the initial temperature
• P2 is the final pressure
• V2 is the final volume
• T2 is the final temperature (unknown)

Plugging the given values into the equation:

(12.4atm)(250ml)/(363K) = (7.1atm)(125ml)/(T2)

Simplifying the equation:

T2 = (7.1atm)(125ml)(363K) / (12.4atm)(250ml)

Solving for T2:

T2 = 484K

Therefore, the final temperature of the gas would be 484 K.