A balloon inflated in a room at 24°C has a volume of 4.00 L. The ballon is then heated to a temperature of 58°C. What is the new volume if the pressure remains constant ?
V1/T1=V2/T24.00/24=X/584.00*58=24*X232/24=X _X=9.6 L
V1/T1=V2/T
24.00/24=X/58
4.00*58=24*X
232/24=X
X=9.6 L
I advise using degrees Kelvin
T1 = 273 + 24 = 297 K
T2 = 273 + 58 = 331
so
V2 = V1 ( T2/T1) = 4 (331/297) = 4.46 Liters
Anonymous is right on. Kelvin is the way to go.
To find the new volume of the balloon when the temperature increases while the pressure remains constant, we can use Charles' Law.
Charles' Law states that the volume of a gas is directly proportional to its absolute temperature when the pressure remains constant.
We can calculate the new volume of the balloon using the formula:
V₁ / T₁ = V₂ / T₂
Where:
V₁ is the initial volume of the balloon
T₁ is the initial temperature
V₂ is the new volume we want to find
T₂ is the new temperature
Given:
V₁ = 4.00 L (initial volume)
T₁ = 24°C + 273.15 (convert to Kelvin)
T₂ = 58°C + 273.15 (convert to Kelvin)
Let's calculate:
V₁ / T₁ = V₂ / T₂
4.00 L / (24°C + 273.15) = V₂ / (58°C + 273.15)
4.00 L / 297.15 K = V₂ / 331.15 K
Now, we can solve for V₂:
V₂ = (4.00 L / 297.15 K) * 331.15 K
V₂ = 4.44 L (rounded to two decimal places)
Therefore, the new volume of the balloon, when heated to a temperature of 58°C while the pressure remains constant, is approximately 4.44 L.