Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Concept explainers
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
![**Balancing Chemical Equations: Understanding the Law of Conservation of Mass**
Balancing chemical equations is a fundamental skill in chemistry. It ensures that the equation adheres to the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. This principle requires the number of atoms for each element to be equal on both sides of the equation.
### Example:
Let's consider the following unbalanced equation:
\[ \text{N}_2 + \text{H}_2 \rightarrow \text{NH}_3 \]
In this equation:
- \(\text{N}_2\) represents nitrogen gas.
- \(\text{H}_2\) represents hydrogen gas.
- \(\text{NH}_3\) represents ammonia.
**Steps to Balance the Equation:**
1. **Identify the number of atoms of each element** on both sides of the equation.
- Reactants: Nitrogen (N) = 2, Hydrogen (H) = 2
- Products: Nitrogen (N) = 1, Hydrogen (H) = 3
2. **Determine the coefficients** that will balance the number of atoms for each element.
- To balance nitrogen (N) atoms, place a coefficient of 2 before \(\text{NH}_3\).
\[ \text{N}_2 + \text{H}_2 \rightarrow 2\text{NH}_3 \]
3. **Balance the hydrogen (H) atoms** by adjusting the coefficients.
- Updating the hydrogen atoms:
- Reactants: Nitrogen (N) = 2, Hydrogen (H) = 2
- Products: Nitrogen (N) = 2, Hydrogen (H) = 6
4. Add a coefficient of 3 before \(\text{H}_2\) to balance the hydrogen atoms.
\[ \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \]
5. **Verify the equation:**
- Reactants: Nitrogen (N) = 2, Hydrogen (H) = 6
- Products: Nitrogen (N) = 2, Hydrogen (H) = 6
The equation is now balanced as there are equal numbers of each type of atom on both sides.
### Important Tips:
- Always start by balancing atoms of elements that appear in only one](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc3c047b-bea2-4c99-927f-560ce831c731%2F4710df1a-eed1-4299-9a31-b3cfc39334ce%2Fx0lyu3_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Balancing Chemical Equations: Understanding the Law of Conservation of Mass**
Balancing chemical equations is a fundamental skill in chemistry. It ensures that the equation adheres to the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. This principle requires the number of atoms for each element to be equal on both sides of the equation.
### Example:
Let's consider the following unbalanced equation:
\[ \text{N}_2 + \text{H}_2 \rightarrow \text{NH}_3 \]
In this equation:
- \(\text{N}_2\) represents nitrogen gas.
- \(\text{H}_2\) represents hydrogen gas.
- \(\text{NH}_3\) represents ammonia.
**Steps to Balance the Equation:**
1. **Identify the number of atoms of each element** on both sides of the equation.
- Reactants: Nitrogen (N) = 2, Hydrogen (H) = 2
- Products: Nitrogen (N) = 1, Hydrogen (H) = 3
2. **Determine the coefficients** that will balance the number of atoms for each element.
- To balance nitrogen (N) atoms, place a coefficient of 2 before \(\text{NH}_3\).
\[ \text{N}_2 + \text{H}_2 \rightarrow 2\text{NH}_3 \]
3. **Balance the hydrogen (H) atoms** by adjusting the coefficients.
- Updating the hydrogen atoms:
- Reactants: Nitrogen (N) = 2, Hydrogen (H) = 2
- Products: Nitrogen (N) = 2, Hydrogen (H) = 6
4. Add a coefficient of 3 before \(\text{H}_2\) to balance the hydrogen atoms.
\[ \text{N}_2 + 3\text{H}_2 \rightarrow 2\text{NH}_3 \]
5. **Verify the equation:**
- Reactants: Nitrogen (N) = 2, Hydrogen (H) = 6
- Products: Nitrogen (N) = 2, Hydrogen (H) = 6
The equation is now balanced as there are equal numbers of each type of atom on both sides.
### Important Tips:
- Always start by balancing atoms of elements that appear in only one
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