Concentration is defined as the amount of substance present in the given space. There are various methods to calculate concentration in chemistry, known as concentration units such as molarity, molality, mass percentage, normality, etc. One of the concentration terms is a mole fraction. In this article, we will study the mole fraction definition and formula in detail.
The mole fraction is the number of molecules in a mixture of a specific component, divided by the total number of moles in that mixture. Mole fraction is a unitless quantity. SymbolÂ â€˜Xâ€™ represents the mole fraction.
Letâ€™s say the components â€˜Aâ€™ and â€˜Bâ€™ are a part of the solution. Then the mole fraction â€˜Xâ€™ can be written as-
â‡’ Mole fraction of component A = \[\frac{\text{no of moles of component A}}{\text{no of moles of component A + no of moles of component B}}\]
Mole fraction formula in chemistry can be written as-
â‡’ X\[_{A}\] = \[\frac{nA}{nA+nB}\]
Here, â€˜Aâ€™ represents the solvent so this equation represents the mole fraction of the solvent formula.
â‡’ Mole fraction of component B = \[\frac{\text{no of moles of component B}}{\text{no of moles of component A + no of moles of component B}}\]
mole fraction formula in chemistry can be written as-
â‡’ X\[_{B}\] = \[\frac{nB}{nA+nB}\]
Here, â€˜Bâ€™ represents the solute so this equation represents the mole fraction of the solute formula.
Therefore, the sum of all the components of the mole fraction is always equal to one.
â‡’ XA+XB=1
If one component of the mole fraction is known then another mole fraction can be calculated.
Lets XA is known then XB can be calculated as-
â‡’ XB=1-XA
It is defined as the pressure exerted by the individual gas in a mixture of gases. Using the mole fraction, the partial pressure of a gas in a mixture can be calculated.
Partial pressure formula with mole fraction:
PA=XAPtotal
Where,
PA= partial pressure of A
XA= mole fraction of A
Ptotal=total partial pressure of a mixture
Example 1: 23g of Ethyl Alcohol is Dissolved in 54g of Water. Calculate the Mole Fraction of Both Ethyl Alcohol and Water in Solution.
Solution: Mass of solute wB=23g
Mass of solvent wA=54g
The molecular formula of ethyl alcohol(C2H5OH)
So, the molar mass of C2H5OH= 12 x 2 + 5 x 1 + 16 + 1Â Â
= 46 g/molÂ
The molecular formula of water(H2O)
So, the molar mass of H2O = 2 x 1 + 16Â
= 18 g/mol
Now, using the formula to find mole fraction-
â‡’ No. of moles of solute(C2H5OH) = nB = 23/46 = 0.5 mol
â‡’ No. of moles of water(H2O) =nA= 54/18 = 3mol
â‡’ Total no. of moles = 0.5 + 3 = 3.5 mol
â‡’ Mole fraction of B component(solute)= XB= 0.5/3.5 = 0.1429
â‡’ Mole fraction of A component(solvent)=XA=3/3.5 = 0.8571
Hence, the mole fraction of component B= 0.1429 and the mole fraction of component A=0.8571
Example 2: The Gas Mixture Comprises 4.76 Moles of Ne, 0.74 Moles of Ar, and 2.5 Moles of Xe. If the Overall Pressure is 2 atm, Measure the Partial Pressure of the Gases. At a Fixed Temperature.
Solution: The total mole fraction of a mixture =4.76+0.74+2.5=8
Using the formula to find mole fraction-
â‡’ XNe= 4.76/8=0.595
â‡’ XAr=0.74/8=0.093
â‡’ XXe=2.5 /8=0.312
Partial pressure-
â‡’ PNe= XNePtotal (total pressure given is 2)
â‡’ PNe= 0.595 x 2= 1.19atm
â‡’ PAr= XArePtotalÂ
â‡’ PAr= 0.093 x 2 = 0.186atm
â‡’ PXe= XXePtotalÂ
â‡’ PXe= 0.312 x 2= 0.624atm
Question: Explain Partial Pressure and Its Importance.
Answer: Partial pressure is the force that a gas exerts. The overall pressure equals the sum of the partial pressures of all the gases in a mixture. In predicting the movement of gases, partial pressure is extremely significant
Question: What's the Difference Between Partial Pressure and Pressure?
Answer: The key difference between the partial pressure and the vapor pressure is that partial pressure is the pressure exerted in a mixture by an individual gas as if it were alone in that environment, while the vapor pressure refers to the pressure exerted by the vapor with its condensed liquid state in its thermodynamic equilibrium
Question: What is the Use of Mole Fraction?
Answer: The mole fraction defines the number of single component molecules (or moles) divided by the total number of molecules (or moles) in the mixture. When two reactive components are mixed together, the mole fraction is useful, as the ratio of the two components is understood if the mole fraction of each is known.
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