A very flexible helium-filled balloon is released from the ground into the air at 20degree C The initial volume of the balloon is 5.00L , and the pressure is 760mmHg. . The balloon ascends to an altitude of 20Km , where the pressure is 76.0mmHg and the temperature is 50degree C What is the new volume,V2 , of the balloon in liters, assuming it doesn't break or leak? plss don't know how to solve this pls if you show me how to do it plsss. thank you
sorry but it should be -50 degree C i typed it wrong
To solve this problem, we can use the combined gas law, which states that the ratio of the initial volume to the final volume is equal to the ratio of the initial pressure to the final pressure, multiplied by the ratio of the final temperature to the initial temperature.
The formula can be written as:
(V1 / V2) = (P1 / P2) * (T1 / T2)
Where:
V1 = initial volume (5.00 L)
V2 = final volume (unknown)
P1 = initial pressure (760 mmHg)
P2 = final pressure (76.0 mmHg)
T1 = initial temperature (20°C + 273.15 = 293.15 K)
T2 = final temperature (50°C + 273.15 = 323.15 K)
Now we can substitute the values into the equation:
V1 / V2 = (P1 / P2) * (T1 / T2)
5.00 L / V2 = (760 mmHg / 76.0 mmHg) * (293.15 K / 323.15 K)
Simplifying further:
5.00 L / V2 = 10 * (293.15 K / 323.15 K)
To isolate V2, divide both sides of the equation by (10 * (293.15 K / 323.15 K)):
V2 = (5.00 L) / (10 * (293.15 K / 323.15 K))
Now we can calculate the value of V2:
V2 = (5.00 L) / (10 * (0.906))
V2 ≈ 0.549 L
Therefore, the new volume of the balloon at an altitude of 20 km is approximately 0.549 liters.