A fixed quantity of gas, at constant pressure, occupies a volume of 8.50 L and has a temperature of 29.0 degrees C. What volume will the gas occupy if the temperature is increased to 125 degrees C?
6.4, 11.2, 14.1, 12.6, 4.9
(V1/T1) = (V2/T2)
T must be in kelvin
To solve this question, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature, assuming constant pressure and amount of gas.
The formula for Charles's Law is V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.
Given:
V1 = 8.50 L
T1 = 29.0 degrees C = 29.0 + 273.15 = 302.15 K (temperature in Kelvin)
Let's find V2:
T2 = 125 degrees C = 125 + 273.15 = 398.15 K
Using the formula V1/T1 = V2/T2:
8.50 L / 302.15 K = V2 / 398.15 K
Now, let's solve for V2:
V2 = (8.50 L / 302.15 K) * 398.15 K
V2 = 11.195 L
Rounded to the nearest tenth, the volume of the gas when the temperature is increased to 125 degrees C is 11.2 L.
Therefore, the answer is 11.2 (option B).