Answer :
To determine how many moles of carbon dioxide (CO₂) can be formed when 4.00 moles of acetylene (C₂H₂) undergo combustion in an excess of oxygen, we first need to consider the balanced chemical equation for the combustion of acetylene:
[tex]\[ \text{C}_2\text{H}_2 + \frac{5}{2} \text{O}_2 \rightarrow 2 \text{CO}_2 + \text{H}_2\text{O} \][/tex]
From the balanced equation, we can observe the following stoichiometric relationship:
- 1 mole of C₂H₂ produces 2 moles of CO₂.
Given:
- You have 4.00 moles of C₂H₂ reacting.
To find out how many moles of CO₂ are produced, you can use the stoichiometric ratio from the equation:
1. Calculate the moles of CO₂:
For every 1 mole of C₂H₂, 2 moles of CO₂ are formed. Therefore, with 4.00 moles of C₂H₂:
[tex]\[
4.00 \, \text{moles of C}_2\text{H}_2 \times \frac{2 \, \text{moles of CO}_2}{1 \, \text{mole of C}_2\text{H}_2} = 8.00 \, \text{moles of CO}_2
\][/tex]
So, 8.00 moles of carbon dioxide are formed when 4.00 moles of acetylene undergo combustion in an excess of oxygen.
[tex]\[ \text{C}_2\text{H}_2 + \frac{5}{2} \text{O}_2 \rightarrow 2 \text{CO}_2 + \text{H}_2\text{O} \][/tex]
From the balanced equation, we can observe the following stoichiometric relationship:
- 1 mole of C₂H₂ produces 2 moles of CO₂.
Given:
- You have 4.00 moles of C₂H₂ reacting.
To find out how many moles of CO₂ are produced, you can use the stoichiometric ratio from the equation:
1. Calculate the moles of CO₂:
For every 1 mole of C₂H₂, 2 moles of CO₂ are formed. Therefore, with 4.00 moles of C₂H₂:
[tex]\[
4.00 \, \text{moles of C}_2\text{H}_2 \times \frac{2 \, \text{moles of CO}_2}{1 \, \text{mole of C}_2\text{H}_2} = 8.00 \, \text{moles of CO}_2
\][/tex]
So, 8.00 moles of carbon dioxide are formed when 4.00 moles of acetylene undergo combustion in an excess of oxygen.
