H_(2)O_(2)arrow H_(2)O+O_(2)

## Step1The given unbalanced chemical equation is: This equation represents the decomposition of hydrogen peroxide ( ) into water ( ) and oxygen gas ( ).## Step2To balance this equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation. This is based on the Law of Conservation of Mass, which states that matter cannot be created or destroyed in a chemical reaction.## Step3Balancing the equation involves adjusting the coefficients (the numbers in front of the chemical formulas) to ensure that the number of atoms of each element is equal on both sides.## Step4The number of hydrogen atoms on the left side is 2 (from ), and it is the same on the right side (from ).## Step5The number of oxygen atoms on the left side is 2 (from ), but on the right side, we have 1 oxygen atom in and 2 in , totaling 3 oxygen atoms.## Step6To balance the oxygen atoms, we can place a coefficient of 2 in front of on the right side. This gives us 2 hydrogen atoms and 2 oxygen atoms on both sides, thus balancing the equation.## Step7The balanced chemical equation is: This balanced equation indicates that two molecules of hydrogen peroxide decompose to form two molecules of water and one molecule of oxygen gas.#