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?

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