The following reaction is balanced. \( \mathrm{KClO}_{3} \rightarrow \mathrm{KCl}+\mathrm{O}_{2} \) True Submit Request Answer

This reaction is indeed not balanced as is. For every two units of potassium chlorate (KClO₃) decomposing, you'd produce two units of potassium chloride (KCl) and three units of oxygen gas (O₂). The balanced equation should be: \( 2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl} + 3 \mathrm{O}_{2} \) Keeping track of the number of each atom on both sides is essential! Balancing chemical equations is like a puzzle! A common mistake is to change subscripts instead of balancing coefficients. Remember, changing subscripts alters the actual compounds involved. Always adjust the coefficients in front of the compounds to maintain the integrity of the reactants and products while ensuring the equation is balanced!