A balloon with an initial volume of 2.8L at a temperature of 296K is warmed to 375K .
What is its volume at the final temperature? (Assume constant pressure.)
To find the volume of the balloon at the final temperature, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature at constant pressure.
Charles's Law equation:
V1 / T1 = V2 / T2
Where:
V1 = Initial volume of the balloon
T1 = Initial temperature of the balloon
V2 = Final volume of the balloon (to be found)
T2 = Final temperature of the balloon
Let's substitute the given values into the equation:
V1 = 2.8 L
T1 = 296 K
T2 = 375 K
Plugging these values into the equation, we get:
2.8 / 296 = V2 / 375
To find V2, let's cross-multiply and solve for V2:
2.8 * 375 = V2 * 296
1050 = V2 * 296
Now, divide both sides by 296 to isolate V2:
1050 / 296 = V2
V2 ≈ 3.54 L
Therefore, the volume of the balloon at the final temperature of 375K is approximately 3.54 liters.
(V1/T1) = (V2/T2)
Remember T must be in kelvin.