Answered: Use the balanced equation to answer the…

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter4: Chemical Reactions

Section: Chapter Questions

Problem 4.63P

See similar textbooks

Related questions

Concept explainers

Question

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?

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Follow-up Questions

Read through expert solutions to related follow-up questions below.

Follow-up Question

Would you be able to show me how to set it up like this? The second image is an example.

**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.

Solution

by Bartleby Expert

SEE SOLUTION

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions