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Chapter 17: Problem 94

How can you tell if a chemical equation is balanced? (Chapter 9\()\)

Short Answer

Expert verified
To determine if a chemical equation is balanced, follow these steps: 1. Identify the elements present in the equation by looking at the reactants and products. 2. Count the atoms of each element on the reactant side and the product side of the equation. 3. Compare the atom counts for each element on both sides of the equation. The equation is balanced if the number of atoms for every element is the same on both the reactant side and the product side. If not, adjust coefficients to balance the equation.

Step by step solution

01

Identify the elements in the equation

First, identify all the elements present in the given chemical equation by looking at the reactants (substances before the arrow) and the products (substances after the arrow). Write down a list of each element and make note of which side of the equation they are on.
02

Count the atoms of each element

For each element listed, count the number of atoms in the reactants and products. Make sure to count the atoms individually, even if they are part of a compound or molecule. Keep a tally for each element on both the reactant and product sides of the equation.
03

Compare the atom counts

Compare the atom counts for each element on both sides of the equation. The chemical equation is balanced if the number of atoms for every element is the same on both the reactant side and the product side.
04

Example: Checking the balance of a chemical equation

As an example, let's analyze the following chemical equation to see if it is balanced: HCl + NaOH 鈫� NaCl + H鈧侽 1. Identify the elements: In this case, we have four elements: hydrogen (H), chlorine (Cl), sodium (Na), and oxygen (O). 2. Count the atoms of each element: - Reactant side: H (1 * 1) = 1, Cl (1 * 1) = 1, Na (1 * 1) = 1, O (1 * 1) = 1 - Product side: H (2 * 1) = 2, Cl (1 * 1) = 1, Na (1 * 1) = 1, O (1 * 1) = 1 3. Compare the atom counts: - Hydrogen: 1 (reactant side) vs 2 (product side) - Chlorine: 1 (reactant side) vs 1 (product side) - Sodium: 1 (reactant side) vs 1 (product side) - Oxygen: 1 (reactant side) vs 1 (product side) Since the number of hydrogen atoms is not equal on both sides of the equation, the original chemical equation is not balanced. To balance this equation, we need to add a coefficient of 2 in front of HCl: 2HCl + NaOH 鈫� NaCl + H鈧侽 Now, the count of hydrogen atoms is the same on both sides, and the equation is balanced.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Reactions
A chemical reaction is a process where one or more substances, known as reactants, are transformed into one or more new substances, known as products. These reactions are essential to chemistry, allowing us to understand how substances change and interact. They can involve various processes such as the breaking of bonds in reactants and the formation of new bonds in products.

Every chemical reaction is unique, and they can vary widely in speed, complexity, and the conditions required for them to occur. Some common signs of a chemical reaction include changes in color, the formation of a gas or solid, or a change in temperature.
  • Reactants: Substances that start a chemical reaction.
  • Products: Substances that are produced by a chemical reaction.
  • Indicators: Changes such as color and temperature that suggest a chemical reaction has taken place.
Understanding chemical reactions is fundamental in fields such as chemistry, biology, and engineering, where they are often used to synthesize new materials or harness energy.
Atoms in Chemical Reactions
In chemical reactions, atoms are immutable 鈥� they aren't created or destroyed, but they can change partners and bonds. This fundamental concept is rooted in the Law of Conservation of Mass, which states that mass is conserved in a chemical reaction.

Atoms in reactants rearrange during a chemical reaction to form products. The number of atoms of each element present in the reaction must remain constant between the reactants and the products.
  • Conservation of Mass: The principle that the total mass of reactants equals the total mass of products, so atoms are not lost in a reaction.
  • Atoms Rearrangement: Atoms shift positions during reactions but no new atoms appear or vanish.
This is why balancing chemical equations is crucial; it ensures that the law of conservation is upheld, reflecting the fact that atoms are simply rearranging to form new products.
Equation Balancing
Balancing chemical equations involves ensuring that the number of each type of atom is equal on both sides of the equation. This practice is crucial because it reflects the real-world principle that in any chemical reaction, atoms are neither created nor destroyed.

When balancing equations, follow these steps:
  • Identify all elements involved in the equation and list them.
  • Count the number of atoms for each element on both sides of the equation.
  • Adjust coefficients (numbers in front of compounds) to make atom counts equal on both sides.
Let's consider an example equation: \( \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \). Notice how initially, the number of hydrogen atoms differs between reactants and products. By adjusting the coefficients, for instance, making it \( 2\text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \), the equation becomes balanced. This shift in the coefficients ensures that the atom count for each element is consistent on both sides, adhering to the law of conservation of mass and atoms.

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Most popular questions from this chapter

Why should you pay attention to the physical states of reactants and products when writing equilibrium constant expressions?

Hard Water The presence of magnesium and calcium ions in water makes the water 鈥渉ard.鈥� Explain in terms of solubility why the presence of these ions is often undesirable. Find out what measures can be taken to eliminate them.

Compare homogeneous and heterogeneous equilibria.

Carbonated Beverages Use Le Ch芒telier's principle to explain how a shift in the equilibrium \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \rightleftharpoons\) \(\mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})\) causes a soft drink to go flat when its container is left open.

How can an equilibrium system contain small and unchanging amounts of products yet have large amounts of reactants? What can you say about the relative size of \(K\) eq for such an equilibrium?
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