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

To find the new volume of helium when pressure changes and temperature remains constant, Boyle's Law is used. The volume increases to 3.79 liters when the pressure decreases from 789 mmHg to 556 mmHg.

Step-by-step explanation:

The student has asked about the change in volume of helium gas in a balloon when the pressure changes while the temperature remains constant. This requires application of Boyle's Law, which states that for a fixed amount of gas at a constant temperature, the volume is inversely proportional to the pressure (P1V1 = P2V2).

We can calculate the new volume V2 of helium when the pressure drops from 789 mmHg to 556 mmHg using the formula:

V2 = (P1 x V1) / P2 = (789 mmHg x 2.68 L) / 556 mmHg = 3.79 L (rounded to two decimal places)

So, the volume of the helium gas increases to 3.79 liters when the pressure decreases to 556 mmHg, assuming the temperature remains unchanged at 23°C.

Answer 2

The volume of helium will be 3.80 L

Step-by-step 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