Homework Help is Here – Start Your Trial Now!
Science
Chemistry
What is the mass in grams of NO that can be formed from 2.18 moles of NO₂ in the reaction below? 3 NO2 (g) + H₂O (g) → 2 HNO3 (g) + NO (g)

What is the mass in grams of NO that can be formed from 2.18 moles of NO₂ in the reaction below? 3 NO2 (g) + H₂O (g) → 2 HNO3 (g) + NO (g)

Chemistry
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...
See similar textbooks
icon
Related questions
Question
100%
**Question 12 of 30** **Problem Statement:** What is the mass in grams of NO that can be formed from 2.18 moles of NO₂ in the reaction below? \[ 3 \, \text{NO}_2 \, (g) + \text{H}_2\text{O} \, (g) \rightarrow 2 \, \text{HNO}_3 \, (g) + \text{NO} \, (g) \] **Explanation:** To determine the mass of NO that can be formed from 2.18 moles of NO₂, we need to follow these steps: 1. **Identify the Stoichiometry of the Reaction:** - According to the balanced chemical equation, 3 moles of NO₂ produce 1 mole of NO. 2. **Calculate Moles of NO Produced:** - From 2.18 moles of NO₂, using the stoichiometry of the reaction (3 moles of NO₂ produce 1 mole of NO), \[ \text{Moles of NO} = \frac{2.18 \, \text{moles of NO}_2}{3} = 0.7267 \, \text{moles of NO} \] 3. **Calculate the Mass of NO:** - The molar mass of NO (Nitric Oxide) is approximately 30.01 g/mol. - Therefore, the mass of NO is calculated as: \[ \text{Mass of NO} = 0.7267 \, \text{moles} \times 30.01 \, \text{g/mol} \approx 21.8 \, \text{g} \] Thus, the mass of NO that can be formed from 2.18 moles of NO₂ is approximately 21.8 grams.
Transcribed Image Text:**Question 12 of 30** **Problem Statement:** What is the mass in grams of NO that can be formed from 2.18 moles of NO₂ in the reaction below? \[ 3 \, \text{NO}_2 \, (g) + \text{H}_2\text{O} \, (g) \rightarrow 2 \, \text{HNO}_3 \, (g) + \text{NO} \, (g) \] **Explanation:** To determine the mass of NO that can be formed from 2.18 moles of NO₂, we need to follow these steps: 1. **Identify the Stoichiometry of the Reaction:** - According to the balanced chemical equation, 3 moles of NO₂ produce 1 mole of NO. 2. **Calculate Moles of NO Produced:** - From 2.18 moles of NO₂, using the stoichiometry of the reaction (3 moles of NO₂ produce 1 mole of NO), \[ \text{Moles of NO} = \frac{2.18 \, \text{moles of NO}_2}{3} = 0.7267 \, \text{moles of NO} \] 3. **Calculate the Mass of NO:** - The molar mass of NO (Nitric Oxide) is approximately 30.01 g/mol. - Therefore, the mass of NO is calculated as: \[ \text{Mass of NO} = 0.7267 \, \text{moles} \times 30.01 \, \text{g/mol} \approx 21.8 \, \text{g} \] Thus, the mass of NO that can be formed from 2.18 moles of NO₂ is approximately 21.8 grams.
Expert Solution
Step 1

Given -

3NO2(g) + H2O(g) -> 2HNO3(g)+ NO(g)

Moles of NO2 =2.18mol

steps

Step by step

Solved in 2 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Stoichiometry
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
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS