81.5k views
5 votes
A sample of gas in a 27.5 L container is initially at 27°C and 725 mmHg. If the pressure is reduced to 457 mmHg and the temperature is increased to 71°C, what is the final volume? Add 273 to convert to Kelvin.

1 Answer

4 votes

Final answer:

The final volume of the gas is 31.72 L.

Step-by-step explanation:

To solve this problem, we can use the combined gas law formula which relates the initial and final values of pressure, volume, and temperature:

P1 * V1 / T1 = P2 * V2 / T2

Plugging in the given values, we have:

(725 mmHg) * (27.5 L) / (27 + 273 K)

= (457 mmHg) * (V2) / (71 + 273 K)

Now, we can solve for V2:

V2 = (725 mmHg * 27.5 L * (71 + 273 K)) / (457 mmHg * (27 + 273 K))

V2 = 31.72 L

Therefore, the final volume of the gas is 31.72 L.

User Duli
by
8.8k points
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.