PV=nRT
P= ? atm
V= 2 L
T= 423 K
n= 2.3 moles
R= 0.08205
(P)(2)=(2.3)(0.08205)(423)
P= (79.826445)/(2)
P= 39.9132225 atm
Start by writing out molar mass of each component:
1) NaOH= 22.99+16+1.01 --> 40
2) Na₃PO₄= (22.99)3 + 94.97 + 64 --> 227.94
3) NaNO₃= 22.99 + 14 + 48 --> 84.99
Now compare the mass of sodium with the rest of the substances:
1) (22.99/40)100%= 57.475%
2) (68.97/227.94)/100%= 30.25%
3) (22.99/84.99)/100%= 27.05%
As seen, the ordered list is: Sodium hydroxide, sodium phosphate and sodium nitrate.
Hope I helped :)
The vapor pressure of the two jars are the same.
The volume of water inside the container does not change the vapor pressure.
As long as the liquid remains being water and the temperature does not change the vapor pressure will be the same. The vapor pressure depends only in the nature of the substance and the temperature of the system.
If you want to know more about this, i.e. why, here you have additional explanation:
The vapor pressure is the pressure of the vapor of a substance in equilibrium with the substance in liquid (or solid state) and it is due to the fact that some molecules in the liquid (or solid), those that are close to the surface of liquid in contact with the gas phase and that have enough kinetic energy, evaporate.
At equilibrium the number of molecules passing from the liquid state to the gas state is equal to the number of molecules that pass from the gas state to the liquid state. If the volume of liquid is increased or decreased, as long as the temperaature of the system remains constant the equilibrium is reached again with the same vapor pressure.
