One more A helium balloon has a volume of 2.30 L at 23.5 deg C and a pressure of 1.00 atm at sea level. the ballon is released and floats upward. At a certain height the atmospheric pressure is 0.810 atm and the temp is 12. C. What is the volume of the balloon? ????? ???
(P1V1/T1 = (P2V2)/T2.
V2 is the unknown. You know all the others.
Don't forget to change T to Kelvin.
K = 273 + C.
Is the answer 2.84??
Close but that isn't the answer I get. Post your work and I'll check it.
To solve this problem, we can use the ideal gas law equation: P1V1/T1 = P2V2/T2, where P1 and P2 are the initial and final pressures, V1 is the initial volume, T1 is the initial temperature, V2 is the final volume (unknown in this case), and T2 is the final temperature.
Given:
P1 = 1.00 atm
V1 = 2.30 L
T1 = 23.5 °C (we need to convert it to Kelvin)
P2 = 0.810 atm
T2 = 12 °C (we also need to convert it to Kelvin)
First, let's convert the temperatures to Kelvin:
T1 = 273 + 23.5 = 296.5 K
T2 = 273 + 12 = 285 K
Now we can substitute the values into the equation and solve for V2:
(1.00 atm)(2.30 L)/(296.5 K) = (0.810 atm)(V2)/(285 K)
Cross-multiplying:
1.00 atm * 2.30 L * 285 K = 0.810 atm * V2 * 296.5 K
Simplifying the equation:
660.45 = 238.25 V2
Finally, solve for V2:
V2 = 660.45/238.25
V2 ≈ 2.77 L
Therefore, the volume of the balloon at the given height is approximately 2.77 L, not 2.84 L as you calculated.