You have a rigid sealed container held at a constant temperature. You add 3.3 atm of oxygen gas, 1.7 atm of nitrogen and 4.2 atm of methane to it. What is the partial pressure of the oxygen gas in the container
Partial pressure does not change.
Partial Pressure of oxygen gas = 3.3 atm
To find the partial pressure of the oxygen gas in the container, you need to know the total pressure inside the container and the mole fraction of oxygen.
The total pressure inside the container is the sum of the partial pressures of all the gases present. In this case, the total pressure is 3.3 atm + 1.7 atm + 4.2 atm = 9.2 atm.
The mole fraction of a gas is the ratio of the number of moles of that gas to the total number of moles of all the gases present.
To find the mole fraction of oxygen, you need to know the number of moles of oxygen gas and the total number of moles of all the gases present. However, this information is not given in the question.
Therefore, without knowing the number of moles of oxygen gas and the total number of moles of all the gases present, it is not possible to determine the partial pressure of the oxygen gas in the container.
If you have the number of moles of each gas, you can use the ideal gas law to find the partial pressure of the oxygen gas. The ideal gas law is given by the equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the gas constant
T is the temperature
By rearranging the equation to solve for the pressure, you can calculate the partial pressure of the oxygen gas.