a 3.0L helium balloon is placed in a car sitting in hot sunlight. The temperature in the mall, when the balloon was bought, was 22C. The temperature in the car is 45C.
what will be the new volume of the of the balloon.
Will it be: 6.14L?
I would think this looks right but the only thing that confuses me, is that I think the volume should actually decrease, not increase.
Please Help
Thanks
Why should it decrease. Charles' Law says that volume increases if T increases. T went from 22 to 45. That's an increase and V should increase. The only think you have done wrong is to use degrees C for temperature. Charles' Law works only for KELVIN.
but is my answer correct?
How can it be correct if you used C instead of Kelvin?
V1/T1= V2/T2
V1 = 3.0 L
V2 = solve for this
T1 = 22 + 273
T2 = 45 + 273
2+2=?
To determine the new volume of the helium balloon, we need to apply the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's convert the temperatures from Celsius to Kelvin:
Initial temperature (in Kelvin) = 22°C + 273.15 = 295.15 K
Final temperature (in Kelvin) = 45°C + 273.15 = 318.15 K
Next, we can use the initial and final temperatures to calculate the ratio of the temperatures:
Temperature ratio = Final temperature / Initial temperature = 318.15 K / 295.15 K
Since the temperature and volume are directly proportional (at constant pressure), we can use the temperature ratio to determine the volume ratio:
Volume ratio = 1 / Temperature ratio = 295.15 K / 318.15 K
To find the new volume of the balloon, we multiply the initial volume by the volume ratio:
New volume = Initial volume * Volume ratio = 3.0 L * (295.15 K / 318.15 K) = 2.768 L (rounded to three decimal places)
Therefore, the new volume of the balloon is approximately 2.768 L, not 6.14 L. The volume decreases due to the increase in temperature.