Question

You fill a balloon with helium gas to a volume of 2.68 L at 23*Cand 789 mmHg. Then you release the balloon. What would be thevolume of helium if its pressure changed to 556 mmHg but thetemperature remained unchanged?

Answer 1

Answer:

The volume of helium will be 3.80 L

Explanation:

Step 1: Data given

Initial volume of the balloon = 2.68 L

Initial temperature of the balloon = 23°C = 296 K

Final temperature of the balloon = 23°C = 296 K

Initial pressure of the balloon = 789 mmHg

Final pressure of the balloon = 556 mmHg

Step 2: Calculate final volume

(P1*V1)/T1 = (P2V2)/T2

(789 * 2.68)/296  = (556*V2)/296

V2 = (789*2.68)/556

V2 = 3.80 L

The volume of helium will be 3.80 L