Question

Balance: ___________ \( \mathrm{NaClO}_{3}$$ \rightarrow\) ___________ \( \mathrm{NaCl}+\) ___________ \(\mathrm{O}_{2}\)

Short answer

The balanced equation is: \( 2 \mathrm{NaClO}_3 \rightarrow 2 \mathrm{NaCl} + 3 \mathrm{O}_2 \).

Step-by-step solution

Write the Unbalanced Equation

To begin, take note of the chemical reaction given: \[ \mathrm{NaClO}_3 \rightarrow \mathrm{NaCl} + \mathrm{O}_2 \] Our objective is to balance the number of atoms for each element on both sides of the equation.

Count Atoms on Each Side

Count the number of sodium (Na), chlorine (Cl), and oxygen (O) atoms in the reactants and products: - Reactants: 1 Na, 1 Cl, 3 O - Products: 1 Na, 1 Cl, 2 O

Balance Oxygen Atoms

Since there are 3 oxygen atoms on the reactant side and 2 on the product side, find the least common multiple of 3 and 2, which is 6. Adjust the coefficients to make the number of oxygen atoms equal:- Use 2 \(\mathrm{NaClO}_3\) and 3 \(\mathrm{O}_2\) on the reactant and product sides, respectively:\[ 2 \mathrm{NaClO}_3 \rightarrow \mathrm{NaCl} + 3 \mathrm{O}_2 \]

Balance Sodium and Chlorine Atoms

Now, there are 2 sodiums and 2 chlorines in the reactants, so place a coefficient of 2 in front of \(\mathrm{NaCl}\):\[ 2 \mathrm{NaClO}_3 \rightarrow 2\, \mathrm{NaCl} + 3 \mathrm{O}_2 \]Thus, the number of Na and Cl atoms are balanced.

Key concepts

Chemical Reactions

Chemical reactions are fascinating transformations that occur when substances interact to form new compounds. These reactions are described by chemical equations, where the substances starting the reaction are called reagents or reactants, and the newly formed substances are termed products.

In the given exercise, the chemical reaction is represented by the equation: \[\mathrm{NaClO}_3\rightarrow \mathrm{NaCl} + \mathrm{O}_2\]This equation shows how sodium chlorate (\(\mathrm{NaClO}_3\)) breaks down into sodium chloride (\(\mathrm{NaCl}\)) and oxygen gas (\(\mathrm{O}_2\)).

Understanding chemical reactions involves recognizing reactants and products as well as describing how atoms are rearranged during the reaction. These reactions are central to the study of chemistry, providing insight into how elements interact to form different compounds in a process filled with energy changes, which could be in form of heat, light, or both.

Stoichiometry

Stoichiometry is a fundamental concept in chemistry that involves calculating the relationships between reactants and products in a chemical reaction. It is based on the conservation of mass principle, where the total mass of reactants equals the total mass of products.

In balancing the chemical equation given in the exercise, stoichiometry is applied to ensure that the number of each type of atom is the same on both sides of the equation. This involves using coefficients to multiply substances in the equation so that:

• The number of sodium (Na) atoms in the reactants equals the number of sodium atoms in the products.
• The number of chlorine (Cl) atoms remains consistent on both sides.
• The number of oxygen (O) atoms is balanced equally across reactants and products.

Stoichiometry provides a quantitative measure that allows chemists to make predictions about the outcome of reactions, estimate reactant quantities required, or determine the amount of products formed.

Through stoichiometry, one can transform a theoretical equation into practical data essential for lab work, industrial applications, and chemical discovery.

Chemical Equation Balancing Steps

Balancing chemical equations is crucial because it adheres to the law of conservation of mass, where total atoms for each element must be the same on both sides of the equation. Here’s how you can easily balance equations using systematic steps:

1. **Identify the Unbalanced Equation:**
Start with the given equation and list out atoms of elements involved. For instance, in the reaction: \[ \mathrm{NaClO}_3 \rightarrow \mathrm{NaCl} + \mathrm{O}_2 \] Identify how many atoms of each element are present in both reactants and products. 2. **Count Atoms for Each Element:**
Tally up sodium (Na), chlorine (Cl), and oxygen (O) atoms. In this example: Reactants:

• 1 Na
• 1 Cl
• 3 O

Products:

• 1 Na
• 1 Cl
• 2 O

3. **Balance Oxygen Atoms First:**
Adjust coefficients to balance oxygen as it appears in both reactants. To balance \(\mathrm{O}_2\), multiply \(\mathrm{NaClO}_3\) by 2 and \(\mathrm{O}_2\) by 3: \[ 2 \mathrm{NaClO}_3 \rightarrow \mathrm{NaCl} + 3 \mathrm{O}_2 \]4. **Balance Sodium and Chlorine Atoms:**
Finally, use a coefficient of 2 for \(\mathrm{NaCl}\) to match the number on the reactants' side: \[ 2 \mathrm{NaClO}_3 \rightarrow 2 \mathrm{NaCl} + 3 \mathrm{O}_2 \]Balancing chemical equations requires patience and practice, but by following these steps methodically, you can accurately equate the number of atoms on both sides, ensuring a balanced and correct chemical equation.