calculate number of dichlorine molecules in a 5.00ml container at 40 degrees Celsius and a pressure of 2.14 x 10^4 Pa.
Use PV = nRT and calculate n = number of mols.
I would use P in atm and volume in L. T must be in kelvin. Then you know that 1 mol contains 6.02E23 molecules; therefore xx mol will contain ?? molecules.
how do i convert Pa to atm?
1 atm = 101.325 kPa
To calculate the number of dichlorine (Cl2) molecules in a given container, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas in Pascals (Pa)
V = volume of the gas in cubic meters (m^3)
n = number of moles of the gas
R = ideal gas constant (8.314 J/(mol·K))
T = temperature of the gas in Kelvin (K)
Let's start by converting the given values to the appropriate units:
Pressure (P) = 2.14 x 10^4 Pa
Volume (V) = 5.00 ml = 5.00 x 10^-6 m^3 (convert milliliters to cubic meters)
Temperature (T) = 40 degrees Celsius = 40 + 273.15 K (convert Celsius to Kelvin)
Now we can plug these values into the ideal gas law equation and solve for the number of moles (n):
n = (PV) / (RT)
n = [(2.14 x 10^4 Pa) * (5.00 x 10^-6 m^3)] / [(8.314 J/(mol·K)) * (40 + 273.15 K)]
Simplifying the equation and canceling units:
n ≈ 0.000416 moles
Finally, we can use Avogadro's number (6.022 x 10^23 molecules/mol) to calculate the number of dichlorine molecules:
Number of molecules = n * Avogadro's number
Number of molecules ≈ 0.000416 moles * (6.022 x 10^23 molecules/mol)
Number of molecules ≈ 2.50 x 10^20 dichlorine molecules
Therefore, there are approximately 2.50 x 10^20 dichlorine molecules in a 5.00 ml container at 40 degrees Celsius and a pressure of 2.14 x 10^4 Pa.