At 0.00 degrees C a 1.00 L flask contains 5.00 x 10^-2 mol N2, 1.50 x 10^2 mg O2, and NH3 at a concentration of 5.00 x 10^18 molecules/mL. What is the partial pressure of each gas, and what is the total pressure in the flask at atm?
Convert mg and molecules to mols.
mols N2 you have.
mols O2 = grams/molar mass = ?
mols NH3 = #molecules/6.02E23 = ?
Use PV = nRT and solve for each pressure.
Then total P = sum of partial pressures.
Thank you very much!
To calculate the partial pressure of each gas in the flask, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(K·mol))
T = temperature (in Kelvin)
Let's calculate the partial pressure of each gas step by step:
1. Convert the given temperature from degrees Celsius to Kelvin:
0.00°C + 273.15 = 273.15 K
2. Convert the given mass of O2 from milligrams to grams:
1.50 x 10^2 mg = 0.150 g
3. Calculate the number of moles of each gas using their respective molar masses:
Molar mass of N2 = 28.0134 g/mol
Number of moles of N2 = 5.00 x 10^-2 mol
Molar mass of O2 = 31.9988 g/mol
Number of moles of O2 = (0.150 g) / (31.9988 g/mol)
4. Calculate the total number of moles of NH3 using the concentration and volume:
Concentration of NH3 = 5.00 x 10^18 molecules/mL
Volume of the flask = 1.00 L
Number of moles of NH3 = (5.00 x 10^18 molecules/mL) * (1.00 L) * (1 mL / 1 x 10^3 L) * (1 mol / 6.022 x 10^23 molecules)
Now we have the number of moles for each gas.
5. Calculate the partial pressure of each gas using the ideal gas law equation:
Partial pressure of N2 = (n * R * T) / V
Partial pressure of O2 = (n * R * T) / V
Partial pressure of NH3 = (n * R * T) / V
6. Calculate the total pressure in the flask by adding the partial pressures of all the gases.
Now that you have all the necessary calculations, you can plug in the values and solve step by step.