a balloon is filled with 500 mL of helium at a temperature of 27 degrees celsius and 755 mmHg as the balloon rises in the atmosphere the pressure and temperature drop what volume will it have when it reaches an altitude where the temperature is -33 degrees celcius and the pressure is 0.65 atm
(P1V1/T1) = (P2V2/T2)
Remember T must be in kelvin.
It's difficult to read sentences, especially in technical areas such as chemistry, when one has a problem knowing where sentences begin and where they end.
BTW, note e the correct spelling of celsius.
I don't get that. Did you use kelvin for both T? Did you convert 0.65 atm to mm Hg (or convert 755 mm Hg to atm?)
Post your work and I'll find the error for you.
To find the final volume of the balloon when it reaches an altitude with a different temperature and pressure, we can use the combined gas law formula.
The combined gas law formula is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume (what we need to find)
T2 = final temperature
Now let's substitute the given values:
P1 = 755 mmHg (convert to atm by dividing by 760 mmHg)
V1 = 500 mL (convert to liters by dividing by 1000 mL)
T1 = 27 degrees Celsius (convert to Kelvin by adding 273.15)
P2 = 0.65 atm
T2 = -33 degrees Celsius (convert to Kelvin by adding 273.15)
Plugging the values into the formula, we have:
(755 mmHg / 760 mmHg) * (500 mL / 1000 mL) / (27 + 273.15) = (0.65 atm * V2) / ( -33 + 273.15)
Simplifying this equation, we get:
V2 = [(755 mmHg / 760 mmHg) * (500 mL / 1000 mL) / (27 + 273.15)] * [(-33 + 273.15) / 0.65 atm]
Now let's solve for V2:
V2 ≈ (0.99342) * (0.49738) * (240.15 / 0.65)
V2 ≈ 90.88518 mL
Therefore, when the balloon reaches the altitude with a temperature of -33 degrees Celsius and pressure of 0.65 atm, it will have a volume of approximately 90.88518 mL.