What is the coefficient in front of the O₂ when the equation below is balanced (using only whole numbers and the lowest whole number ratio)? C2H6O2(g) + O₂ (g) → CO₂(g) + H₂O (g)

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### Balancing Chemical Equations

**Question:**
What is the coefficient in front of the \( \text{O}_2 \) when the equation below is balanced (using only whole numbers and the lowest whole number ratio)?

**Given Equation:**
\[ \text{C}_2\text{H}_6\text{O}_2(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O(g)} \]

In order to balance this chemical equation, follow these steps:

1. **Count the number of atoms of each element on both sides of the equation.**

   - Left side (Reactants):
     - C (Carbon): 2
     - H (Hydrogen): 6
     - O (Oxygen): 4 (from \( \text{C}_2\text{H}_6\text{O}_2 \)) + 2x (from \( \text{O}_2 \))

   - Right side (Products):
     - C (Carbon): 1x (from \( \text{CO}_2 \))
     - H (Hydrogen): 2y (from \( \text{H}_2\text{O} \))
     - O (Oxygen): 2x (from \( \text{CO}_2 \)) + y (from \( \text{H}_2\text{O} \))

2. **Balance the atoms of each element one at a time, using coefficients.**

   - Balance Carbon (C):
     - Since there are 2 Carbons in the reactants (\( \text{C}_2\text{H}_6\text{O}_2 \)), put a coefficient of 2 in front of \( \text{CO}_2 \).
     \[ \text{C}_2\text{H}_6\text{O}_2(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) + \text{H}_2\text{O(g)} \]

   - Balance Hydrogen (H):
     - There are 6 Hydrogens in the reactants (\( \text{C}_2\text{H}_6\text{O}_2 \)), so put a coefficient of 3 in front of \( \text{H}_2\
Transcribed Image Text:### Balancing Chemical Equations **Question:** What is the coefficient in front of the \( \text{O}_2 \) when the equation below is balanced (using only whole numbers and the lowest whole number ratio)? **Given Equation:** \[ \text{C}_2\text{H}_6\text{O}_2(g) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O(g)} \] In order to balance this chemical equation, follow these steps: 1. **Count the number of atoms of each element on both sides of the equation.** - Left side (Reactants): - C (Carbon): 2 - H (Hydrogen): 6 - O (Oxygen): 4 (from \( \text{C}_2\text{H}_6\text{O}_2 \)) + 2x (from \( \text{O}_2 \)) - Right side (Products): - C (Carbon): 1x (from \( \text{CO}_2 \)) - H (Hydrogen): 2y (from \( \text{H}_2\text{O} \)) - O (Oxygen): 2x (from \( \text{CO}_2 \)) + y (from \( \text{H}_2\text{O} \)) 2. **Balance the atoms of each element one at a time, using coefficients.** - Balance Carbon (C): - Since there are 2 Carbons in the reactants (\( \text{C}_2\text{H}_6\text{O}_2 \)), put a coefficient of 2 in front of \( \text{CO}_2 \). \[ \text{C}_2\text{H}_6\text{O}_2(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) + \text{H}_2\text{O(g)} \] - Balance Hydrogen (H): - There are 6 Hydrogens in the reactants (\( \text{C}_2\text{H}_6\text{O}_2 \)), so put a coefficient of 3 in front of \( \text{H}_2\
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