A sample of air has a volume of 140.0 mL at 67 Degrees Celsius.?
At what temperature will its volume be 50.0 mL at constant pressure?
I don't understand what the question is asking how to set up the euation can someone explain
Certainly! To solve this problem, you can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature when pressure is held constant. The equation for Charles's Law is:
V1 / T1 = V2 / T2
Where:
V1 is the initial volume (in mL),
T1 is the initial temperature (in Kelvin),
V2 is the final volume (in mL), and
T2 is the final temperature (in Kelvin).
Now, let's set up the equation using the given information:
Given:
Initial volume (V1) = 140.0 mL
Initial temperature (T1) = 67 degrees Celsius
Final volume (V2) = 50.0 mL (the volume we want to find)
Final temperature (T2) = ?
First, let's convert the initial temperature from degrees Celsius to Kelvin. The Kelvin scale is obtained by adding 273.15 to the Celsius value. So, 67 degrees Celsius + 273.15 = 340.15 K.
Now, we can substitute the known values into Charles's Law equation:
140.0 mL / 340.15 K = 50.0 mL / T2
To solve for T2, we need to rearrange the equation:
T2 = (50.0 mL * 340.15 K) / 140.0 mL
T2 ≈ 122.2 K
Therefore, at constant pressure, the air sample will have a volume of 50.0 mL at a temperature of approximately 122.2 Kelvin.