Balance The Following Equation:$\[ C_3H_{12} + O_2 \rightarrow CO_2 + H_2O \\]Select The Coefficient That Would Go In Front Of $\[ O_2 \\].A. 6 B. 5 C. 8 D. 16

Introduction

Balancing chemical equations is a crucial concept in chemistry that helps us understand the stoichiometry of chemical reactions. It is essential to balance chemical equations to ensure that the law of conservation of mass is obeyed, which states that matter cannot be created or destroyed in a chemical reaction. In this article, we will focus on balancing the equation $C_3H_{12} + O_2 \rightarrow CO_2 + H_2O$ and select the correct coefficient for $O_2$.

Understanding the Equation

The given equation is:

$$C_3H_{12} + O_2 \rightarrow CO_2 + H_2O$$

This equation represents a combustion reaction, where a hydrocarbon ($C_3H_{12}$) reacts with oxygen ($O_2$) to produce carbon dioxide ($CO_2$) and water ($H_2O$).

Step 1: Count the Atoms

To balance the equation, we need to count the number of atoms of each element on both the reactant and product sides. Let's start with the reactant side:

• Carbon (C): 3 atoms
• Hydrogen (H): 12 atoms
• Oxygen (O): 2 atoms (from $O_2$)

Now, let's count the number of atoms on the product side:

• Carbon (C): 1 atom (from $CO_2$)
• Hydrogen (H): 2 atoms (from $H_2O$)
• Oxygen (O): 3 atoms (2 from $CO_2$ and 1 from $H_2O$)

Step 2: Balance the Carbon Atoms

Since there are 3 carbon atoms on the reactant side, we need to multiply the $CO_2$ molecule by 3 to balance the carbon atoms:

$$C_3H_{12} + O_2 \rightarrow 3CO_2 + H_2O$$

Step 3: Balance the Hydrogen Atoms

Now, let's balance the hydrogen atoms. There are 12 hydrogen atoms on the reactant side, and we have 2 hydrogen atoms on the product side. To balance the hydrogen atoms, we need to multiply the $H_2O$ molecule by 6:

$$C_3H_{12} + O_2 \rightarrow 3CO_2 + 6H_2O$$

Step 4: Balance the Oxygen Atoms

Finally, let's balance the oxygen atoms. There are 2 oxygen atoms on the reactant side, and we have 9 oxygen atoms on the product side (6 from $6H_2O$ and 3 from $3CO_2$). To balance the oxygen atoms, we need to multiply the $O_2$ molecule by 9/2, which is not a whole number. However, we can multiply the $O_2$ molecule by 4.5, which is not a whole number either. Since we cannot have a fraction of a molecule, we need to multiply the entire equation by 2 to get rid of the fraction:

$$2C_3H_{12} + 7O_2 \rightarrow 6CO_2 + 12H_2O$$

Conclusion

In conclusion, the balanced equation is:

$$2C_3H_{12} + 7O_2 \rightarrow 6CO_2 + 12H_2O$$

The correct coefficient for $O_2$ is 7.

Discussion

Balancing chemical equations is a crucial concept in chemistry that helps us understand the stoichiometry of chemical reactions. It is essential to balance chemical equations to ensure that the law of conservation of mass is obeyed. In this article, we focused on balancing the equation $C_3H_{12} + O_2 \rightarrow CO_2 + H_2O$ and selected the correct coefficient for $O_2$. We also discussed the importance of balancing chemical equations and provided a step-by-step guide on how to balance chemical equations.

Common Mistakes

When balancing chemical equations, it is essential to avoid common mistakes such as:

• Not counting the atoms correctly
• Not balancing the atoms in the correct order (e.g., balancing the carbon atoms before balancing the hydrogen atoms)
• Not multiplying the entire equation by a whole number to get rid of fractions

Tips and Tricks

When balancing chemical equations, here are some tips and tricks to keep in mind:

• Always count the atoms correctly
• Balance the atoms in the correct order
• Multiply the entire equation by a whole number to get rid of fractions
• Use a systematic approach to balance the equation (e.g., balance the atoms in the order of their atomic mass)

Conclusion

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Introduction

Balancing chemical equations is a crucial concept in chemistry that helps us understand the stoichiometry of chemical reactions. In our previous article, we provided a step-by-step guide on how to balance the equation $C_3H_{12} + O_2 \rightarrow CO_2 + H_2O$. In this article, we will answer some frequently asked questions about balancing chemical equations.

Q: What is the law of conservation of mass?

A: The law of conservation of mass states that matter cannot be created or destroyed in a chemical reaction. This means that the total mass of the reactants must equal the total mass of the products.

Q: Why is it essential to balance chemical equations?

A: Balancing chemical equations is essential to ensure that the law of conservation of mass is obeyed. It also helps us understand the stoichiometry of chemical reactions, which is crucial in chemistry.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, follow these steps:

1. Count the number of atoms of each element on both the reactant and product sides.
2. Balance the atoms in the correct order (e.g., balance the carbon atoms before balancing the hydrogen atoms).
3. Multiply the entire equation by a whole number to get rid of fractions.
4. Check that the law of conservation of mass is obeyed.

Q: What are some common mistakes to avoid when balancing chemical equations?

A: Some common mistakes to avoid when balancing chemical equations include:

• Not counting the atoms correctly
• Not balancing the atoms in the correct order
• Not multiplying the entire equation by a whole number to get rid of fractions

Q: How do I know if a chemical equation is balanced?

A: A chemical equation is balanced if the number of atoms of each element on both the reactant and product sides is equal. You can check this by counting the number of atoms of each element on both sides of the equation.

Q: Can I balance a chemical equation by trial and error?

A: While it is possible to balance a chemical equation by trial and error, it is not the most efficient way to do so. A systematic approach to balancing chemical equations is recommended.

Q: What are some tips and tricks for balancing chemical equations?

A: Some tips and tricks for balancing chemical equations include:

• Always count the atoms correctly
• Balance the atoms in the correct order
• Multiply the entire equation by a whole number to get rid of fractions
• Use a systematic approach to balance the equation (e.g., balance the atoms in the order of their atomic mass)

Q: Can I use a calculator to balance a chemical equation?

A: While a calculator can be useful in balancing chemical equations, it is not always necessary. A systematic approach to balancing chemical equations can be done without a calculator.

Conclusion

Balancing chemical equations is a crucial concept in chemistry that helps us understand the stoichiometry of chemical reactions. In this article, we answered some frequently asked questions about balancing chemical equations. We also provided some tips and tricks for balancing chemical equations. By following these tips and tricks, you can become proficient in balancing chemical equations.

Common Questions

• Q: What is the difference between a balanced and unbalanced chemical equation? A: A balanced chemical equation has the same number of atoms of each element on both the reactant and product sides, while an unbalanced chemical equation does not.
• Q: Can I balance a chemical equation with a negative coefficient? A: No, you cannot balance a chemical equation with a negative coefficient.
• Q: How do I balance a chemical equation with a fraction? A: To balance a chemical equation with a fraction, multiply the entire equation by a whole number to get rid of the fraction.

Additional Resources

• Balancing Chemical Equations Worksheet: A worksheet with practice problems on balancing chemical equations.
• Balancing Chemical Equations Video: A video tutorial on balancing chemical equations.
• Balancing Chemical Equations Online Tool: An online tool that can help you balance chemical equations.