Question

drag each number to the correct location on the equation. each number can be used more than once, but not all numbers will be used. balance the equation with the correct coefficients. 2 3 4 5 kclo₃ → kcl + o₂ reset next

Explanation:

Step1: Balance O atoms

On the left, \( \text{KClO}_3 \) has 3 O atoms. On the right, \( \text{O}_2 \) has 2 O atoms. The least common multiple of 3 and 2 is 6. So, we need 2 \( \text{KClO}_3 \) (giving 6 O atoms) and 3 \( \text{O}_2 \) (also giving 6 O atoms).

$$2\text{KClO}_3 ightarrow \text{KCl} + 3\text{O}_2$$

Step2: Balance K and Cl atoms

Now, with 2 \( \text{KClO}_3 \), we have 2 K and 2 Cl atoms on the left. So, we need 2 \( \text{KCl} \) on the right.

$$2\text{KClO}_3 ightarrow 2\text{KCl} + 3\text{O}_2$$

Answer:

The balanced equation is \( \boldsymbol{2}\text{KClO}_3
ightarrow \boldsymbol{2}\text{KCl} + \boldsymbol{3}\text{O}_2 \)