Question

a weather balloon contains 450L helium at 25C and 765 mmHg. what is the volume of the balloon when it ascends to an altitude where the temperature is 2C and the pressure is 650 mmHg?

Answer 1

Step-by-step explanation:

We can solve this problem using the combined gas law, which states that:

(P1 × V1) / T1 = (P2 × V2) / T2

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.

We are given:

P1 = 765 mmHg

V1 = 450 L

T1 = 25°C + 273.15 = 298.15 K

We need to find V2.

We can convert the final temperature to Kelvin:

T2 = 2°C + 273.15 = 275.15 K

Now we can plug in the values:

(765 mmHg × 450 L) / 298.15 K = (650 mmHg × V2) / 275.15 K

Solving for V2:

V2 = (765 mmHg × 450 L × 275.15 K) / (298.15 K × 650 mmHg)

≈ 570.26 L

Therefore, the volume of the balloon when it ascends to the new altitude is approximately 570.26 L.