2. Ammonium perchlorate reacts with aluminum according to the balanced reaction below. 3 NHACIO. (s) + 3 Al (s)→3 NO(g) + 1 Al2O(s) + 6H₂O(g) +1 AIC (g) a. If 67.1 g of ammonium perchlorate were to react with 10.0 g of aluminum, which substance would be the limiting reactant? b. How many liters of each gaseous product are formed, if the reaction occurs at STP? C. How many grams of excess reactant remains after the reaction is complete?
2. Ammonium perchlorate reacts with aluminum according to the balanced reaction below. 3 NHACIO. (s) + 3 Al (s)→3 NO(g) + 1 Al2O(s) + 6H₂O(g) +1 AIC (g) a. If 67.1 g of ammonium perchlorate were to react with 10.0 g of aluminum, which substance would be the limiting reactant? b. How many liters of each gaseous product are formed, if the reaction occurs at STP? C. How many grams of excess reactant remains after the reaction is complete?
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...
Related questions
Question
Please answer this asap and include all the steps please.
![**Reaction of Ammonium Perchlorate with Aluminum**
In this section, we will explore a chemical reaction involving ammonium perchlorate and aluminum. The balanced chemical equation for this reaction is provided below:
\[ 3 \text{NH}_4\text{ClO}_4(s) + 3 \text{Al} (s) \rightarrow 3 \text{NO} (g) + 1 \text{Al}_2\text{O}_3(s) + 6 \text{H}_2\text{O} (g) + 1 \text{AlCl}_3(g) \]
**Problem Statement:**
a. If 67.1 g of ammonium perchlorate were to react with 10.0 g of aluminum, which substance would be the limiting reactant?
b. How many liters of each gaseous product are formed, if the reaction occurs at STP?
c. How many grams of excess reactant remains after the reaction is complete?
**Detailed Breakdown:**
1. **Determine the Limiting Reactant:**
- Calculate the molar masses of NH4ClO4 and Al.
- Convert the given masses of NH4ClO4 and Al to moles.
- Use stoichiometry to determine which reactant is limiting based on the balanced equation proportions.
2. **Volume of Gaseous Products:**
- Identify the gaseous products from the equation.
- Calculate the total moles of each gaseous product using the limiting reactant.
- Convert the moles of gases to volume at STP (Standard Temperature and Pressure) using the ideal gas law (1 mole of gas = 22.4 liters at STP).
3. **Excess Reactant Remaining:**
- Calculate how much of the excess reactant is consumed in the reaction using stoichiometry.
- Subtract the consumed amount from the original amount to find the remaining mass of the excess reactant.
This exercise illustrates fundamental concepts in stoichiometry, limiting reactants, ideal gas law calculations, and conservation of mass in chemical reactions. These concepts are essential for a solid understanding of chemical reactions and their quantitative aspects.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9359044e-f021-4fc6-a0ad-5a2dc758cf44%2F44d1b2e2-77e6-4f62-afb1-e5497667caa5%2Fagdkxjo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Reaction of Ammonium Perchlorate with Aluminum**
In this section, we will explore a chemical reaction involving ammonium perchlorate and aluminum. The balanced chemical equation for this reaction is provided below:
\[ 3 \text{NH}_4\text{ClO}_4(s) + 3 \text{Al} (s) \rightarrow 3 \text{NO} (g) + 1 \text{Al}_2\text{O}_3(s) + 6 \text{H}_2\text{O} (g) + 1 \text{AlCl}_3(g) \]
**Problem Statement:**
a. If 67.1 g of ammonium perchlorate were to react with 10.0 g of aluminum, which substance would be the limiting reactant?
b. How many liters of each gaseous product are formed, if the reaction occurs at STP?
c. How many grams of excess reactant remains after the reaction is complete?
**Detailed Breakdown:**
1. **Determine the Limiting Reactant:**
- Calculate the molar masses of NH4ClO4 and Al.
- Convert the given masses of NH4ClO4 and Al to moles.
- Use stoichiometry to determine which reactant is limiting based on the balanced equation proportions.
2. **Volume of Gaseous Products:**
- Identify the gaseous products from the equation.
- Calculate the total moles of each gaseous product using the limiting reactant.
- Convert the moles of gases to volume at STP (Standard Temperature and Pressure) using the ideal gas law (1 mole of gas = 22.4 liters at STP).
3. **Excess Reactant Remaining:**
- Calculate how much of the excess reactant is consumed in the reaction using stoichiometry.
- Subtract the consumed amount from the original amount to find the remaining mass of the excess reactant.
This exercise illustrates fundamental concepts in stoichiometry, limiting reactants, ideal gas law calculations, and conservation of mass in chemical reactions. These concepts are essential for a solid understanding of chemical reactions and their quantitative aspects.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 5 steps with 5 images
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY