A 1.00 L volume of helium gas is cooled from 50.0 degrees celcius to 25.0 degrees celcius. If the pressure remains constant, what is the final volume?
V1/T1 = V2/T2
Don't forget to use T in Kelvin.
(and note the correct spelling of celsius).
To find the final volume of the helium gas, you can use the ideal gas law, which states:
PV = nRT
Where:
P is the pressure (which remains constant in this case)
V is the volume (what we are trying to find)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L*atm/(mol*K))
T is the temperature in Kelvin
Since the pressure is constant, the equation simplifies to:
V1/T1 = V2/T2
Where:
V1 and T1 are the initial volume and temperature, respectively
V2 and T2 are the final volume and temperature, respectively.
First, we need to convert the temperatures from Celsius to Kelvin:
T1 = 50.0 + 273.15 = 323.15 K
T2 = 25.0 + 273.15 = 298.15 K
Now we can plug these values into the equation:
V1/T1 = V2/T2
V1/323.15 = V2/298.15
To find V2 (the final volume), rearrange the equation:
V2 = (V1 * T2) / T1
Substituting the given values:
V2 = (1.00 L * 298.15 K) / 323.15 K
Calculating the final volume, we get:
V2 = 0.922 L
Therefore, the final volume of the helium gas is 0.922 L.