Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. Ca, (PO), (s) + SiO₂ (s) + C(s) → CaSiO₂ (s) + P(s) + CO(g) 1 X ?
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. Ca, (PO), (s) + SiO₂ (s) + C(s) → CaSiO₂ (s) + P(s) + CO(g) 1 X ?
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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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: An Example**
Chemical equations represent the reactants and products in a chemical reaction. To adhere to the Law of Conservation of Mass, these equations must be balanced, meaning the same number of atoms for each element must be present on both sides of the equation. Here is an example of balancing a chemical equation:
**Prompt:**
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients:
\[ \text{Ca}_3(\text{PO}_4)_2 (\text{s}) + \text{SiO}_2 (\text{s}) + \text{C} (\text{s}) \rightarrow \text{CaSiO}_3 (\text{s}) + \text{P}_4 (\text{s}) + \text{CO} (\text{g}) \]
**Explanation:**
To balance this equation, follow these steps:
1. **Identify each element in the equation.**
2. **Tally the number of atoms of each element in both the reactants and products.**
Reactants:
- \( \text{Ca}_3(\text{PO}_4)_2 \):
- \(\text{Ca}=3, \text{P}=2, \text{O}=8\)
- \(\text{SiO}_2\):
- \(\text{Si}=1, \text{O}=2\)
- \(\text{C}\):
- \(\text{C}=1\)
Products:
- \(\text{CaSiO}_3\):
- \(\text{Ca}=1, \(\text{Si}=1, \(\text{O}=3\)
- \(\text{P}_4\):
- \(\text{P}=4\)
- \(\text{CO}\):
- \(\text{C}=1, \(\text{O}=1\)
3. **Balance one element at a time by adjusting coefficients.** Use the smallest possible whole numbers as coefficients.
- Balance Calcium (Ca):
\[ \text{Ca}_3(\text{PO}_4)_2: \text{Ca}=3 \rightarrow 3\text{CaSiO}_3: \text{Ca}=3 \]
- Balance Phosphorus (P):
\[ \text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2869f911-fc69-4f3e-bbf4-69a25f43f41f%2Fb9e6f82d-ce6c-4d17-bdf8-072eb7d53f1a%2F98v4jam_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Balancing Chemical Equations: An Example**
Chemical equations represent the reactants and products in a chemical reaction. To adhere to the Law of Conservation of Mass, these equations must be balanced, meaning the same number of atoms for each element must be present on both sides of the equation. Here is an example of balancing a chemical equation:
**Prompt:**
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients:
\[ \text{Ca}_3(\text{PO}_4)_2 (\text{s}) + \text{SiO}_2 (\text{s}) + \text{C} (\text{s}) \rightarrow \text{CaSiO}_3 (\text{s}) + \text{P}_4 (\text{s}) + \text{CO} (\text{g}) \]
**Explanation:**
To balance this equation, follow these steps:
1. **Identify each element in the equation.**
2. **Tally the number of atoms of each element in both the reactants and products.**
Reactants:
- \( \text{Ca}_3(\text{PO}_4)_2 \):
- \(\text{Ca}=3, \text{P}=2, \text{O}=8\)
- \(\text{SiO}_2\):
- \(\text{Si}=1, \text{O}=2\)
- \(\text{C}\):
- \(\text{C}=1\)
Products:
- \(\text{CaSiO}_3\):
- \(\text{Ca}=1, \(\text{Si}=1, \(\text{O}=3\)
- \(\text{P}_4\):
- \(\text{P}=4\)
- \(\text{CO}\):
- \(\text{C}=1, \(\text{O}=1\)
3. **Balance one element at a time by adjusting coefficients.** Use the smallest possible whole numbers as coefficients.
- Balance Calcium (Ca):
\[ \text{Ca}_3(\text{PO}_4)_2: \text{Ca}=3 \rightarrow 3\text{CaSiO}_3: \text{Ca}=3 \]
- Balance Phosphorus (P):
\[ \text
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