A 19.3L expandible container is filled in a room where the pressure is 761mmHg. It is filled with 600.4mmHg nitrogen, 108mmHg oxygen, 32.1 mmHg water vapor. The rest of the pressure is made up by carbon dioxide. The temperature is 20.3°C
a. What is the partial pressure of carbon dioxide?
b. What is the mass of carbon dioxide?
c. If this container is connected to a sealed 24.0L container that is filled with 761 mmHg of Ne (T = 20.3°) and opened, what is the total pressure inside the combined container and the partial pressure of Ne?
i think A is 20.5mmhg and B is .951 g CO2 are these right and im not sure how to start C
A is right. B is right.
C.
I would calculate n for each of the gases. You know partial pressure of each, V, R, & T from the first container.
Mols Ne can be calculated from P Ne, V of the second container, R & T.
Find total mols, use that with R, & T and total volume to find total pressure when the two containers are connected.
Partial pressure Ne from the combined containers is pNe = XNe*Ptotal. (XNe = mols Ne/total mols)
thank you very much
To solve these questions, we can use the ideal gas law, which states that the product of pressure (P) and volume (V) is directly proportional to the number of moles (n) of a gas and the ideal gas constant (R) multiplied by the temperature (T).
a. To find the partial pressure of carbon dioxide (CO2), we need to first calculate the mole fraction of CO2 in the mixture.
1. Calculate the mole fraction of each gas:
The mole fraction (X) of a gas is the ratio of the number of moles of that gas to the total number of moles.
Mole fraction of nitrogen (N2):
n(N2) = 600.4 mmHg / 760 mmHg * 19.3 L / 0.0821 L•atm/K•mol * (273.15 + 20.3) K
= 0.4726 mol
Mole fraction of oxygen (O2):
n(O2) = 108 mmHg / 760 mmHg * 19.3 L / 0.0821 L•atm/K•mol * (273.15 + 20.3) K
= 0.0844 mol
Mole fraction of water vapor (H2O):
n(H2O) = 32.1 mmHg / 760 mmHg * 19.3 L / 0.0821 L•atm/K•mol * (273.15 + 20.3) K
= 0.0252 mol
Total number of moles (n_total):
n_total = n(N2) + n(O2) + n(H2O)
= 0.4726 mol + 0.0844 mol + 0.0252 mol
= 0.5822 mol
2. Calculate the mole fraction of carbon dioxide (CO2):
X(CO2) = (n_total - n(N2) - n(O2) - n(H2O)) / n_total
Substituting the values, we find:
X(CO2) = 0.5822 mol / 0.5822 mol
= 1
Since the mole fraction of CO2 is 1, the partial pressure of CO2 is equal to the remaining pressure in the container when considering nitrogen, oxygen, and water vapor pressures.
Partial pressure of carbon dioxide (P(CO2)) = Total pressure - (Pressure of N2 + Pressure of O2 + Pressure of H2O)
P(CO2) = (761 mmHg - 600.4 mmHg - 108 mmHg - 32.1 mmHg)
= 20.5 mmHg
Therefore, the partial pressure of carbon dioxide is 20.5 mmHg.
b. To find the mass of carbon dioxide (CO2), we need to know the number of moles of CO2 and the molar mass of CO2.
1. Calculate the number of moles of CO2:
n(CO2) = X(CO2) * n_total
= 1 * 0.5822 mol
= 0.5822 mol
2. Calculate the molar mass of CO2:
The molar mass of CO2 can be found by adding the atomic masses of carbon and oxygen:
Molar mass of CO2 = (12.01 g/mol) + 2 * (16.00 g/mol)
= 44.01 g/mol
3. Calculate the mass of CO2:
Mass of CO2 = n(CO2) * molar mass of CO2
Substituting the values, we find:
Mass of CO2 = 0.5822 mol * 44.01 g/mol
= 25.59 g
Therefore, the mass of carbon dioxide is 25.59 g.
c. To determine the total pressure inside the combined container and the partial pressure of neon (Ne), we can use Dalton's law of partial pressures. This law states that the total pressure exerted by a mixture of gases is equal to the sum of their partial pressures.
1. Calculate the total number of moles in the combined container:
n_ne = 761 mmHg * 24.0 L / 0.0821 L·atm/K·mol * (273.15 + 20.3) K
2. Calculate the total number of moles in the combined container:
n_total = n_total_CO2 + n_ne
3. Calculate the total pressure in the combined container using the ideal gas law:
P_total = (n_total * R * T) / V_total
4. Calculate the partial pressure of neon (P_Ne) using the mole fraction (X_Ne):
P_Ne = X_Ne * P_total
Substituting the values, you can find the total pressure and the partial pressure of neon in the combined container.
Note: To calculate the mole fraction of neon (X_Ne), you can use the formula:
X_Ne = n_ne / (n_total_CO2 + n_ne)
You can now follow the steps outlined above to calculate the remaining values.