as we define mole to be mass of the solute divided by molecular mass of the solute so all the solutes are taken in the solid form not in the liquid like we take 1L in molarity,so solids are generally independent of temp thats why both molality and mole fraction are independent of temperature
because mole fraction doesnot depend on volume
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
10 to the power of 7?
Dependent variable: growth of crystals Independent variable: temperature.
temperature(it is whats changed on purpose)
because mole fraction doesnot depend on volume
For Ideal gases, mole fraction=volume fraction
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
The mole fraction of Oxygen = 21/100= .21
The mole fraction of HCl is 0.34.
Phase diagrams usually show phase transition boundaries relative to two variables. WHICH two variables depends on what they're trying to show, but usually is is two of the following: Temperature Pressure Volume/density Mole fraction Mass fraction ========== PT PV less commonly - TV Isobaric T vs mole fraction (e.g. melting point diagram) Isothermal P vs mole fraction (e.g. a vapor pressure diagram)
the mole fraction of oxygen= 37/100 0.37 the mole fraction of Nitrogen= .63 that equals to give 1
Mole fraction is dimensionless. It's the amount of moles of species "A" divided by the total amount of moles in the mixture. So "mole A / mole total" equals "dimensionless". To add clarity in the use of mole fractions, one could add as "unit" mole A / mole "mixture".
The mole fraction of HCl in 20 percent aqueous solution is 0.21.
The molar mass of benzene (C6H6) is 78.11 grams per mole. The molar mass of toluene is 92.14 grams per mole. Mole fraction of a solute equals moles of solute divided by the moles of solute plus the moles of solvent. .5 of each is the mole fraction.
Relative lowering of vapour pressure is function of pressure of pure liquid and pressure of solutions when you increase temperature both the values increase and compensate the increase value, According to the Raoult's law, Psolvent = Xsolvent Po where Psolvent is the vapour pressure of the liquid solution, Xsolvent is its mole fraction in the solution and Po is the pure vapour pressure.
Relative lowering of vapour pressure is function of pressure of pure liquid and pressure of solutions when you increase temperature both the values increase and compensate the increase value, According to the Raoult's law, Psolvent = Xsolvent Po where Psolvent is the vapour pressure of the liquid solution, Xsolvent is its mole fraction in the solution and Po is the pure vapour pressure.