A gas is trapped in a balloon. The gas chambee is 1.0 atm, the volume is 0.066 L, and the temperature is 298 K. When the temperature is changed to 308 K and the pressure remains constant, what is the new volume of the balloon?
(V1/T1) = (V2/T2)
Don't forget T must be in kelvin.
To solve this problem, we can use Charles' Law, which states that the volume of a gas is directly proportional to its absolute temperature, assuming constant pressure.
The equation for Charles' Law is: V₁/T₁ = V₂/T₂
Given:
Initial volume (V₁) = 0.066 L
Initial temperature (T₁) = 298 K
New temperature (T₂) = 308 K (temperature is changed to this value)
Pressure (P) remains constant
To find the new volume (V₂), we rearrange the equation and solve for V₂:
V₂ = (V₁ × T₂) / T₁
Substituting the values:
V₂ = (0.066 L × 308 K) / 298 K
Now, let's calculate the new volume:
V₂ = (0.020328 L)
Therefore, the new volume of the balloon, when the temperature is changed to 308 K and the pressure remains constant, is approximately 0.020 L.