Mole Concept formulas
Master Mole Concept through 22 JEE Advanced-level formulas, systematically structured with every variable spelled out. Revise concept-wise, identify the areas where you need improvement, and focus your preparation with greater precision.
Mole Concept, every formula
22 formulas, typeset and free. Print it, or keep it open beside your practice.
Number of moles (mass)
Q1NumericalMoles from massThe number of moles in $36$ g of water (M=18) is:Number of particles
N_A = 6.022×10²³
Q1MCQNumber of particlesThe number of molecules in $2$ mol of a gas is:- A$2N_A$
- B$\dfrac{N_A}{2}$
- C$N_A$
- D$4N_A$
- A
Moles from volume (gas, STP)
at STP
Q1NumericalGas volume STPThe number of moles in $11.2$ L of a gas at STP is:Avogadro's number
Q1MCQAvogadro numberAvogadro's number is approximately:- A$6.022\times10^{23}$
- B$6.022\times10^{-23}$
- C$3.011\times10^{23}$
- D$1.6\times10^{-19}$
- A
Molar mass of a gas
Q1NumericalMolar massIf $8$ g of a gas is $0.25$ mol, its molar mass (g/mol) is:Mole fraction
Q1NumericalMole fractionA mixture has $2$ mol A and $3$ mol B. The mole fraction of A is (decimal):Molarity
Q1NumericalMolarity$0.5$ mol of NaCl in $2$ L of solution has molarity:Molality
Q1NumericalMolality$1$ mol of solute in $500$ g of solvent has molality (mol/kg):Normality
Q1MCQNormalityNormality is defined as:- A$\dfrac{\text{gram equivalents}}{\text{volume (L)}}$
- B$\dfrac{\text{moles}}{\text{volume}}$
- C$\dfrac{\text{moles}}{\text{mass}}$
- D$M\times V$
- A
Normality–molarity relation
Q1NumericalN = M × n-factorA $2$ M $H_2SO_4$ solution (n-factor 2) has normality:Equivalent weight
Q1NumericalEquivalent weightThe equivalent weight of $H_2SO_4$ (M=98, n-factor 2) is:Percentage by mass
Q1Numerical% by mass$10$ g of solute in $50$ g of solution has percentage by mass:ppm
Q1Numericalppm$2$ mg of solute in $1$ kg of solution corresponds to (in ppm):Empirical formula mass relation
Q1MCQMolecular formulaThe molecular formula is related to the empirical formula by:- Amolecular $=n\times$ empirical
- Bmolecular $=$ empirical
- Cmolecular $=\dfrac{\text{empirical}}{n}$
- Dunrelated
- A
Molecular formula factor
Q1Numericaln factor (mol formula)A compound has empirical formula mass $30$ and molar mass $60$. The multiplier $n$ is:Dilution
Q1NumericalDilution$100$ mL of $2$ M solution is diluted to $400$ mL. The new molarity (M) is:Mixing solutions
Q1NumericalMixingMixing $1$ L of $2$ M and $1$ L of $4$ M gives molarity (M):Vapour density
Q1NumericalVapour densityA gas has vapour density $16$. Its molar mass (g/mol) is:Average atomic mass
isotopic abundance
Q1MCQAverage atomic massThe average atomic mass is:- A$\sum x_i A_i$
- B$\sum A_i$
- C$\dfrac{\sum A_i}{n}$
- D$\max A_i$
- A
Law of definite proportions
Q1MCQDefinite proportionsThe law of definite proportions states that a compound has:- Aa fixed mass ratio of its elements
- Bvariable composition
- Cequal atoms of each element
- Dno fixed formula
- A
Limiting reagent
Q1MCQLimiting reagentIn a reaction, the amount of product is decided by the:- Alimiting reagent
- Bexcess reagent
- Ccatalyst
- Dsolvent
- A
Atoms in a molecule
Q1NumericalAtoms countThe number of oxygen atoms in $1$ mol of $O_2$ (in units of $N_A$) is:
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