A 2.5 L sample of gas at 25 degrees Celsius is heated to 50 degrees celcius at constant pressure. What would the volume be at 50 degrees celcius?
(V1/T1) = (V2/T2)
T must be in kelvin
To calculate the volume of the gas at 50 degrees Celsius, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, let's convert the temperatures from Celsius to Kelvin. The Kelvin temperature scale doesn't have negative values, so we add 273.15 to the Celsius temperature:
Initial temperature (T1) = 25 + 273.15 = 298.15 K
Final temperature (T2) = 50 + 273.15 = 323.15 K
Since the pressure is constant, we can express the equation as V1/T1 = V2/T2, where V1 is the initial volume and V2 is the desired volume.
Now let's substitute the known values into the equation:
V1/T1 = V2/T2
V1 = 2.5 L (The initial volume)
T1 = 298.15 K (Initial temperature)
T2 = 323.15 K (Final temperature)
Now we can solve for V2:
(2.5 L) / (298.15 K) = V2 / (323.15 K)
Cross multiplying:
(2.5 L) * (323.15 K) = V2 * (298.15 K)
805.375 L⋅K = V2 * (298.15 K)
Divide both sides by 298.15 K:
805.375 L⋅K / 298.15 K = V2
V2 ≈ 2.70 L
Therefore, the volume of the gas at 50 degrees Celsius would be approximately 2.70 liters.