Assume the volume of a filter flask is 250.0mL. You have added (25.0 + 10.0)mL of solution so the volume of gas is (250.0 - 35.0) = 215.0mL. Calculate the extra volume of gas forced into the burette because of the measured average temperature of 23 degrees Celsius.
To calculate the extra volume of gas forced into the burette due to the measured average temperature of 23 degrees Celsius, we need to use the ideal gas law equation:
V2 = V1 * (T2/T1)
where:
V1 = initial volume of gas (215.0 mL)
T1 = initial temperature (assumed to be in Kelvin)
T2 = final temperature (23 degrees Celsius + 273.15)
First, we need to convert the initial temperature to Kelvin:
T1 = 273.15 + 23 = 296.15 K
Now we can plug the values into the equation:
V2 = 215.0 mL * (296.15 K / T2)
Let's calculate the extra volume of gas forced into the burette for the given temperature:
V2 = 215.0 mL * (296.15 K / (23 degrees Celsius + 273.15))
V2 = 215.0 mL * (296.15 K / 296.15 K)
V2 = 215.0 mL
Therefore, the extra volume of gas forced into the burette due to the measured average temperature of 23 degrees Celsius is 215.0 mL.
To calculate the extra volume of gas forced into the burette due to the measured average temperature of 23 degrees Celsius, we need to use the Ideal Gas Law.
The Ideal Gas Law is expressed as:
PV = nRT
Where:
P = Pressure (in Pascals)
V = Volume (in cubic meters)
n = Number of moles
R = Ideal Gas Constant (8.314 J/(mol⋅K))
T = Temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin. To do that, we add 273.15 to the temperature in Celsius.
Temperature in Kelvin = (23 + 273.15) = 296.15 K
Next, we need to convert the volume from mL to cubic meters. Since 1 mL is equal to 1e-6 cubic meters, we can calculate the volume as follows:
Volume in cubic meters = 215.0 mL * 1e-6 m^3/mL = 0.000215 m^3
Now, let's rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / (RT)
Assuming the pressure is constant, we can substitute the pressure with 1 atm, which is equal to 101,325 Pa.
n = (1 atm * 0.000215 m^3) / (8.314 J/(mol⋅K) * 296.15 K)
Calculating this, we get:
n ≈ 8.21e-6 mol
Since we know the volume of the excess gas is the difference between the initial volume and the volume of the solution added:
Excess volume of gas = (250.0 mL - (25.0 mL + 10.0 mL)) * 1e-6 m^3/mL
Excess volume of gas ≈ 215.00 mL * 1e-6 m^3/mL
Excess volume of gas ≈ 0.000215 m^3
Finally, we can calculate the extra volume of gas forced into the burette using the number of moles and the ideal gas law:
Extra volume of gas forced into the burette = nRT / P
Assuming the pressure in the burette is 1 atm, we can calculate:
Extra volume of gas forced into the burette = (8.21e-6 mol * 8.314 J/(mol⋅K) * 296.15 K) / (1 atm * 101,325 Pa * 0.000215 m^3)
Calculating this, we get:
Extra volume of gas forced into the burette ≈ 0.125 mL
Therefore, the extra volume of gas forced into the burette due to the measured average temperature of 23 degrees Celsius is approximately 0.125 mL.