Use the balanced equation to answer the question follows. 2C2H6(g)+5O2(g) -----> 4CO(g)+6H2O(g) to calculate how many moles of O2 are needed to react completely with 1.6 moles of C2H6?
Use the balanced equation to answer the question follows. 2C2H6(g)+5O2(g) -----> 4CO(g)+6H2O(g) to calculate how many moles of O2 are needed to react completely with 1.6 moles of C2H6?
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Use the balanced equation to answer the question follows. 2C2H6(g)+5O2(g) -----> 4CO(g)+6H2O(g) to calculate how many moles of O2 are needed to react completely with 1.6 moles of C2H6?
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![**Conversion Factors in Chemical Reactions**
---
**Example Problem:**
Determine the number of moles of \(O_2\) required to react with a given quantity of \(C_2H_6\) (ethane).
**Balanced Chemical Equation:**
\[ 2C_2H_6(g) + 5O_2(g) \rightarrow 4CO(g) + 6H_2O(g) \]
**Given Quantity:**
\[ 1.6 \text{ moles of } C_2H_6 \]
**Units Desired:**
\[ \text{moles of } O_2 \]
**Conversion Factors:**
To solve this problem, use stoichiometry based on the balanced chemical equation to convert from moles of \(C_2H_6\) to moles of \(O_2\). The conversion factor can be derived from the coefficients in the balanced equation.
---
The reaction shows that 2 moles of \(C_2H_6\) react with 5 moles of \(O_2\).
\[
\left( \frac{5 \text{ moles of } O_2}{2 \text{ moles of } C_2H_6} \right)
\]
Using this conversion factor, you can calculate the moles of \(O_2\) needed for 1.6 moles of \(C_2H_6\).](https://content.bartleby.com/qna-images/question/9a7b46e8-8a33-44cb-988f-05793dec8601/48fafa52-bc42-42d0-9e1c-45e3c079d056/gmnq3em_processed.jpeg)
Transcribed Image Text:**Conversion Factors in Chemical Reactions**
---
**Example Problem:**
Determine the number of moles of \(O_2\) required to react with a given quantity of \(C_2H_6\) (ethane).
**Balanced Chemical Equation:**
\[ 2C_2H_6(g) + 5O_2(g) \rightarrow 4CO(g) + 6H_2O(g) \]
**Given Quantity:**
\[ 1.6 \text{ moles of } C_2H_6 \]
**Units Desired:**
\[ \text{moles of } O_2 \]
**Conversion Factors:**
To solve this problem, use stoichiometry based on the balanced chemical equation to convert from moles of \(C_2H_6\) to moles of \(O_2\). The conversion factor can be derived from the coefficients in the balanced equation.
---
The reaction shows that 2 moles of \(C_2H_6\) react with 5 moles of \(O_2\).
\[
\left( \frac{5 \text{ moles of } O_2}{2 \text{ moles of } C_2H_6} \right)
\]
Using this conversion factor, you can calculate the moles of \(O_2\) needed for 1.6 moles of \(C_2H_6\).
![### Stoichiometry Calculation for Ethane to Carbon Dioxide
#### 1. Problem Statement
**Given:**
- Mass of Ethane (\(C_2H_6\)) = 100.0 g
**Find:**
- Mass of Carbon Dioxide (\(CO_2\)) produced
#### 2. Solution Process
#### **Quantity Calculation**
\[
100.0 \, \text{g} \, C_2H_6 \times \frac{1 \, \text{mole} \, C_2H_6}{30 \, \text{g} \, C_2H_6} \times \frac{4 \, \text{moles CO}_2}{2 \, \text{moles} \, C_2H_6} \times \frac{44 \, \text{g CO}_2}{1 \, \text{mole CO}_2} = \textcolor{#ff0000}{293 \, \text{g CO}_2}
\]
#### **Conversion Factors**
1. **From Stoichiometric Equation:**
\[
2 \, \text{moles} \, C_2H_6 = 4 \, \text{moles CO}_2
\]
2. **From Molecular Weight of \(C_2H_6\):**
\[
1 \, \text{mole} \, C_2H_6 = 30 \, \text{g} \, C_2H_6
\]
3. **From Molecular Weight of \(CO_2\):**
\[
1 \, \text{mole CO}_2 = 44 \, \text{g CO}_2
\]
These conversion factors are used in the calculation to determine the mass of \(CO_2\) produced from the given mass of \(C_2H_6\).
#### **Final Answer:**
\[
\boxed{293 \, \text{g CO}_2}
\]
The mass of carbon dioxide (\(CO_2\)) produced from 100.0 g of ethane (\(C_2H_6\)) is 293 g.](https://content.bartleby.com/qna-images/question/9a7b46e8-8a33-44cb-988f-05793dec8601/48fafa52-bc42-42d0-9e1c-45e3c079d056/bvznxap_processed.jpeg)
Transcribed Image Text:### Stoichiometry Calculation for Ethane to Carbon Dioxide
#### 1. Problem Statement
**Given:**
- Mass of Ethane (\(C_2H_6\)) = 100.0 g
**Find:**
- Mass of Carbon Dioxide (\(CO_2\)) produced
#### 2. Solution Process
#### **Quantity Calculation**
\[
100.0 \, \text{g} \, C_2H_6 \times \frac{1 \, \text{mole} \, C_2H_6}{30 \, \text{g} \, C_2H_6} \times \frac{4 \, \text{moles CO}_2}{2 \, \text{moles} \, C_2H_6} \times \frac{44 \, \text{g CO}_2}{1 \, \text{mole CO}_2} = \textcolor{#ff0000}{293 \, \text{g CO}_2}
\]
#### **Conversion Factors**
1. **From Stoichiometric Equation:**
\[
2 \, \text{moles} \, C_2H_6 = 4 \, \text{moles CO}_2
\]
2. **From Molecular Weight of \(C_2H_6\):**
\[
1 \, \text{mole} \, C_2H_6 = 30 \, \text{g} \, C_2H_6
\]
3. **From Molecular Weight of \(CO_2\):**
\[
1 \, \text{mole CO}_2 = 44 \, \text{g CO}_2
\]
These conversion factors are used in the calculation to determine the mass of \(CO_2\) produced from the given mass of \(C_2H_6\).
#### **Final Answer:**
\[
\boxed{293 \, \text{g CO}_2}
\]
The mass of carbon dioxide (\(CO_2\)) produced from 100.0 g of ethane (\(C_2H_6\)) is 293 g.
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