ChemistrySome basic concepts of chemistryClass 11

Mole concept and limiting reagent: interactive simulation

Molarity uses litres of solution. Molality uses kilograms of solvent, so heating the solution does not change it. The limiting reagent is the one that can make less product.

Useful for: JEE Main, JEE Advanced, NEET, CBSE Boards · 2 modes in one lab

What you can explore

  1. 1

    Molarity, molality, mole fraction

    One mass of solute, three different concentration units.
  2. 2

    Limiting reagent

    N₂ + 3H₂ → 2NH₃. The bar that runs out first sets the yield.

Try this

  1. 1

    Keep the solute fixed and increase only the solution volume.

    What you should see

    Molarity falls. Molality does not, because the water mass did not change.

  2. 2

    Set 2 mol N₂ and 3 mol H₂.

    What you should see

    H₂ is limiting. Only 2 mol of NH₃ can form.

Formulas behind it

Molarity

M=nVLM = \frac{n}{V_{\text{L}}}

Molality

m=nkg solventm = \frac{n}{\text{kg solvent}}

Mole fraction

x=nn+nsolventx = \frac{n}{n + n_{\text{solvent}}}

Common mistakes

  • Using the solution volume in the molality formula, or the solvent mass in the molarity formula.
Stuck on a mole concept and limiting reagent question?Snap it and get a whiteboard video solution.

FAQ

Which reagent is limiting when 1 mol N₂ meets 3 mol H₂?

Neither. The ratio is exactly 1 : 3, so both are used up.

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