Question

A helium-filled weather balloon has a volume of 697 L at 22.9°C and 754 mmHg. It is released and rises to an altitude of 6.93 km, where the pressure is 377 mmHg and the temperature is –23.1°C. The volume of the balloon at this altitude is L.

Answer 1

The new volume at this altitude is 1177.3 L

Step-by-step explanation:

Step 1: Data given

Volume of a helium filled balloon = 697 L

Temperature = 22.9 °C = 295.9 K

Pressure = 754 mmHg

The pressure reduces to 377 mmHg

The temperature decreases to -23.1 °C = 249.9 K

Step 2: Calculate the new volume at this altitude

P1 *V1 / T1 = P2*V2 / T2

⇒with P1 = the initial pressure of the gas = 754 mmHg

⇒with V1 = the initial volume in the balloon = 697 L

⇒with T1 = the initial volume = 295.9 K

⇒with P2 = the reduced pressure = 377 mmHg

⇒with V2 = the new volume = TO BE DETERMINED

⇒with T2 = the decreased temperature = 249.9 K

(754 mmHg* 697 L ) / 295.9 K = (377 mmHg * V2) / 249.9 K

V2 = 1177.3 L

The new volume at this altitude is 1177.3 L

Answer 2

1412.2L is the new volume

Step-by-step explanation:

Given

Volume V1= 697l

Volume V2=?

Temperature t1= 22.9°c

Temperature t2=23.2°c

Pressure P1=754mmHg

Pressure P2=377mmHg

Using.

P1V1/T1=P2V2/T2

V2=P1V1T2/T1P2

754*697*23.2/22.9*377

V2=1412.2l