Cu(OH)₂ → CuO + H₂O

Decomposition of copper(II) hydroxide — balanced chemical equation, step by step.

Blue copper(II) hydroxide turns to black copper(II) oxide when heated, a common classroom colour change.

How to balance Cu(OH)2 = CuO + H2O

A decomposition reaction breaks one compound down into two or more simpler substances. Balancing means choosing coefficients so that every element has the same number of atoms on both sides of the arrow — the Law of Conservation of Mass. Here is how it's done, step by step.

Step 1 — Write the unbalanced equation

Start with the correct formulas for every reactant and product:

Cu(OH)2 = CuO + H2O

Step 2 — Count the atoms of each element

Counting the atoms on each side, every element already matches — so each coefficient is 1:

Step 3 — Add the smallest whole-number coefficients

Adjust the coefficients in front of each formula until every element balances. The smallest whole-number coefficients are 1 Cu(OH)₂, 1 CuO, 1 H₂O, giving:

Cu(OH)2 = CuO + H2O

For a decomposition reaction, balance the element common to the fewest products first, then work outward to the simpler substances.

Step 4 — Verify the balance

Recount every element. Each one now matches on both sides:

All elements are balanced and the coefficients are the smallest whole numbers, so Cu(OH)2 = CuO + H2O is the correct balanced equation.

Molar masses and mole ratio

The balanced coefficients are also the mole ratio of the reaction. Using standard atomic masses, the molar mass of each substance is:

For this reaction the mole ratio is 1 : 1 : 1. Combine these molar masses with the ratio in the free stoichiometry calculator to convert between moles, grams, and the number of particles for any reactant or product.

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