### Stoichiometry Problem: Calculating the Mass of NO#### Problem Statement:What is the mass in grams of NO that can be formed from 7.26 moles of NO₂ in the reaction below?\[ 3 \text{NO}_2 (g) + \text{H}_2\text{O} (g) \rightarrow 2 \text{HNO}_3 (g) + \text{NO} (g) \]#### Introduction:This problem involves the stoichiometric calculation of the mass of nitrogen monoxide (NO) produced from a given amount of nitrogen dioxide (NO₂). The balanced chemical equation provides the mole ratio necessary for this calculation.#### Procedure:1. **Identify the Mole Ratio**: From the balanced reaction, 3 moles of NO₂ produce 1 mole of NO.2. **Calculate Moles of NO**: Using the given moles of NO₂: \[ \frac{7.26 \text{ moles NO}_2}{3 \text{ moles NO}_2} = 2.42 \text{ moles NO} \]3. **Calculate Mass of NO**: The molar mass of NO is approximately 30 g/mol. So, the mass of NO formed is: \[ 2.42 \text{ moles NO} \times 30 \text{ g/mol} = 72.6 \text{ g} \]### Conclusion:Given 7.26 moles of NO₂, 72.6 grams of NO can be produced under the conditions described by the balanced chemical equation.#### Interface Details:- **Calculator Interface**: The problem appears on an educational platform with an integrated calculator interface for inputting numerical data and performing calculations.- **Graphical Elements**: There are no graphical elements or diagrams associated with this problem. The focus is on understanding and applying the stoichiometric relationships described in the equation.

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What is the mass in grams of NO that can be formed from 7.26 moles of NO₂ in the reaction below? 3 NO₂ (g) + H₂O (g) → 2 HNO3 (g) + NO (g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

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### Stoichiometry Problem: Calculating the Mass of NO

#### Problem Statement:
What is the mass in grams of NO that can be formed from 7.26 moles of NO₂ in the reaction below?

\[ 3 \text{NO}_2 (g) + \text{H}_2\text{O} (g) \rightarrow 2 \text{HNO}_3 (g) + \text{NO} (g) \]

#### Introduction:
This problem involves the stoichiometric calculation of the mass of nitrogen monoxide (NO) produced from a given amount of nitrogen dioxide (NO₂). The balanced chemical equation provides the mole ratio necessary for this calculation.

#### Procedure:
1. **Identify the Mole Ratio**: From the balanced reaction, 3 moles of NO₂ produce 1 mole of NO.

2. **Calculate Moles of NO**:
Using the given moles of NO₂:
\[
\frac{7.26 \text{ moles NO}_2}{3 \text{ moles NO}_2} = 2.42 \text{ moles NO}
\]

3. **Calculate Mass of NO**:
The molar mass of NO is approximately 30 g/mol. So, the mass of NO formed is:
\[
2.42 \text{ moles NO} \times 30 \text{ g/mol} = 72.6 \text{ g}
\]

### Conclusion:
Given 7.26 moles of NO₂, 72.6 grams of NO can be produced under the conditions described by the balanced chemical equation.

#### Interface Details:
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- **Graphical Elements**: There are no graphical elements or diagrams associated with this problem. The focus is on understanding and applying the stoichiometric relationships described in the equation.

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