11 posts • Page 1 of 1
Partial pressure just means that it is a part/contributing to the total pressure of the system. Total pressure is all of the components of a reaction that would cause pressure combined (added), while partial pressure is just the pressure created by one aspect or compound.
For a gas phase reaction, we express equilibrium constant by pressures, and when there is 1 gas it is the total pressure whereas 2 more gases are referred to as partial gas of each gas implying that the sum of them will make up the total pressure.
The total pressure is the pressure of the entire system, whereas each gas making up the system has its own partial pressure, which makes up the total pressure. If you had a container with O2 and H2 gas is it and the partial pressure of each gas was 0.5 atm, the total pressure would be 1 atm.
Partial pressure is the pressure of an individual type of gas molecule within a gas mixture. The total pressure is the combined pressure of all the gases making up the gas mixture. Therefore, the total pressure is equal to the sum of all of the partial pressures for each type of gas in the gas mixture. Partial pressure is proportional to its mole fraction. An example: If there are 4 moles of O2 and 6 moles of N2 and the total pressure is 10 atm, then what is the partial pressure of O2? Since O2 has a mole fraction of 4 atm / 10 atm = 0.4, it has a partial pressure of 0.4(10 atm) = 4 atm.
Who is online
Users browsing this forum: No registered users and 1 guest