Answer :
Certainly! Let's solve this step-by-step.
The balanced chemical equation for the combustion of methane (CH₄) is:
[tex]\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \][/tex]
This equation tells us that:
- 1 mole of CH₄ produces 1 mole of CO₂.
- 1 mole of CH₄ also produces 2 moles of H₂O.
This establishes a stoichiometric relationship between CO₂ and H₂O:
- For every 1 mole of CO₂ formed, 2 moles of H₂O are formed.
Given: 0.15 moles of H₂O are formed.
Let's find out how many moles of CO₂ are formed.
1. Using the stoichiometric relationship:
[tex]\[ \frac{2 \text{ moles of H}_2\text{O}}{1 \text{ mole of CO}_2} \][/tex]
2. We want to find the number of moles of CO₂ (let's call it x) when 0.15 moles of H₂O are formed.
Thus, using the ratio:
[tex]\[ 2 \text{ moles of H}_2\text{O} \text{ form 1 mole of CO}_2 \][/tex]
[tex]\[ \text{0.15 moles of H}_2\text{O forms } \frac{0.15}{2} = 0.075 \text{ moles of CO}_2 \][/tex]
So, 0.15 moles of H₂O will result in 0.075 moles of CO₂ being formed.
The balanced chemical equation for the combustion of methane (CH₄) is:
[tex]\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \][/tex]
This equation tells us that:
- 1 mole of CH₄ produces 1 mole of CO₂.
- 1 mole of CH₄ also produces 2 moles of H₂O.
This establishes a stoichiometric relationship between CO₂ and H₂O:
- For every 1 mole of CO₂ formed, 2 moles of H₂O are formed.
Given: 0.15 moles of H₂O are formed.
Let's find out how many moles of CO₂ are formed.
1. Using the stoichiometric relationship:
[tex]\[ \frac{2 \text{ moles of H}_2\text{O}}{1 \text{ mole of CO}_2} \][/tex]
2. We want to find the number of moles of CO₂ (let's call it x) when 0.15 moles of H₂O are formed.
Thus, using the ratio:
[tex]\[ 2 \text{ moles of H}_2\text{O} \text{ form 1 mole of CO}_2 \][/tex]
[tex]\[ \text{0.15 moles of H}_2\text{O forms } \frac{0.15}{2} = 0.075 \text{ moles of CO}_2 \][/tex]
So, 0.15 moles of H₂O will result in 0.075 moles of CO₂ being formed.
