Science

Common mistakes in chemical calculations and moles

4 mistakes learners make with chemical calculations and moles, each one named and explained.

All common mistakes

A mole is a fixed number of particles, so the same mass of two different substances is not the same number of particles.

Equal masses taken to be equal numbers of particles

What it looks like

You say 10 g of hydrogen and 10 g of oxygen contain the same number of molecules.

Why it happens

Mass is the quantity you can see on the balance, so it stands in for amount.

A worked example

Question. Which contains more molecules, 16 g of methane or 16 g of oxygen?

A common answer. they contain the same number

The answer. the methane, because its molecules are lighter

Why. Lighter molecules means more of them fit into the same mass.

Put the two side by side

The same mass can hide very different numbers of particles.
The same number of moles is the same number of particles.

Convert to moles before comparing amounts. Mass alone does not count particles.

Mass expected to stay the same when a gas escapes

What it looks like

You say the mass cannot change because nothing was added or taken away, even though the container is open.

Why it happens

Mass is conserved is the rule you have learned, and a gas leaving is invisible.

A worked example

Question. Marble chips react with acid in an open flask. What happens to the mass?

A common answer. it stays the same, because mass is conserved

The answer. it falls, because carbon dioxide leaves the flask

Why. Mass is conserved overall, but the gas carrying it has left the flask you are weighing.

Put the two side by side

Mass is conserved in the reaction.
Mass measured on the balance falls if a gas gets out.

Ask whether anything can leave. Conservation applies to everything, not to the flask.

The big number and the small number read the same way

What it looks like

You count the atoms in 2H2O as 2 hydrogens and 1 oxygen, or as 2 of each.

Why it happens

Both numbers are written near the letters, and only one of them is read aloud in class.

A worked example

Question. How many hydrogen atoms are in 2H2O?

A common answer. 2

The answer. 4

Why. The 2 in front multiplies the whole formula, and each H2O holds 2 hydrogens.

Put the two side by side

The small number counts atoms inside one molecule.
The big number counts the molecules.

Multiply the two together for the atom count, every time.

The formula changed to make an equation balance

What it looks like

You change a small number inside a formula, turning H2O into H2O2, so the oxygens come out even.

Why it happens

The subscripts are the numbers in front of you when the atoms do not match, so they look like the ones to adjust.

A worked example

Question. Balance: H2 + O2 gives H2O

A common answer. H2 + O2 gives H2O2

The answer. 2H2 + O2 gives 2H2O

Why. Changing a subscript makes a different substance. Only the big numbers in front may change.

Put the two side by side

A subscript names the substance.
A number in front counts how many of it you have.

Never touch a subscript. Balance with the big numbers only.

WAJD spots these patterns in your child's answers and names the one behind their wrong answers, instead of just marking them wrong.

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