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
To solve this problem, we will need to use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
a. To find the partial pressure of carbon dioxide (CO2), we need to subtract the sum of the partial pressures of nitrogen (N2), oxygen (O2), and water vapor (H2O) from the total pressure.
Partial pressure of CO2 = Total pressure - (Partial pressure of N2 + Partial pressure of O2 + Partial pressure of H2O)
First, we need to convert all the pressures to the same units. Since the total pressure is given in mmHg, we will convert the partial pressures of N2, O2, and H2O to mmHg.
Partial pressure of N2 = 600.4 mmHg
Partial pressure of O2 = 108 mmHg
Partial pressure of H2O = 32.1 mmHg
Now we can calculate the partial pressure of CO2:
Partial pressure of CO2 = 761 mmHg - (600.4 mmHg + 108 mmHg + 32.1 mmHg)
b. To find the mass of carbon dioxide (CO2), we need to determine the number of moles of CO2 and then multiply it by the molar mass of CO2.
First, let's calculate the number of moles of CO2. We can use the ideal gas law equation to find this:
PV = nRT
Rearranging the equation to solve for n:
n = PV / RT
Using the known values:
Partial pressure of CO2 = [calculated in part (a)]
Volume (V) = 19.3 L
Temperature (T) = 20.3°C + 273.15 K (to convert to Kelvin)
Ideal gas constant (R) = 0.0821 L·atm/(mol·K)
Now we can calculate the number of moles of CO2:
n = (Partial pressure of CO2 * V) / (R * T)
Once we have the number of moles of CO2, we can find the mass using the molar mass of CO2, which is approximately 44.01 g/mol.
Mass of CO2 = Number of moles of CO2 * Molar mass of CO2
c. To solve part (c), we need to calculate the total pressure inside the combined container and the partial pressure of Ne. Since the two containers are connected and the system is sealed, the total number of moles will remain constant. We can use the ideal gas law equation again to find the total pressure.
First, we'll calculate the number of moles of Ne in the second container using:
n = PV / RT
Where:
Partial pressure of Ne = 761 mmHg
Volume (V) = 24.0 L
Temperature (T) = 20.3°C + 273.15 K (to convert to Kelvin)
Ideal gas constant (R) = 0.0821 L·atm/(mol·K)
After finding the number of moles of Ne, we can add it to the number of moles of CO2 from part (b). Then, we can use the total number of moles to calculate the total pressure inside the combined container.
Remember to convert all pressures to the same unit, such as mmHg or atm, before performing calculations.