A gas occupied 224 L at 25 c . At what temperature would this gas occupy 164 liters pressure constants
(V1/T1) = (V2/T2)
What is the temperature in Celsius of a gas that will occupy 46.5L at 2.56 atm?
To solve this problem, we can use the combined gas law equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 = initial pressure (constant pressure, so we can skip this term)
V1 = initial volume = 224 L
T1 = initial temperature = 25 °C + 273.15 (convert to Kelvin)
P2 = final pressure (constant pressure, so we can skip this term)
V2 = final volume = 164 L
T2 = final temperature (what we need to find)
First, let's convert the initial temperature to Kelvin:
T1 = 25 °C + 273.15 = 298.15 K
Now let's rearrange the equation to solve for T2:
T2 = (P2 * V2 * T1) / (P1 * V1)
Since the pressure is constant (P1 = P2), we can cancel out those terms:
T2 = (V2 * T1) / V1
Now, substitute the given values:
T2 = (164 L * 298.15 K) / 224 L
Calculate the result:
T2 = 217.82 K
Therefore, the gas would occupy 164 liters at a temperature of approximately 217.82 Kelvin.