The compound NH4CI can be decomposcd to form NH3 and HCI. This can be represented at the atomic level by a chemical equation: NH,CI NH3 + HCI According to the law of conservation of mass, if 28.5 grams of NH,Cl decomposes and 9.1 grams of NH3 is formed, how many grams of HCI must simultaneously be formed? | grams HCl
The compound NH4CI can be decomposcd to form NH3 and HCI. This can be represented at the atomic level by a chemical equation: NH,CI NH3 + HCI According to the law of conservation of mass, if 28.5 grams of NH,Cl decomposes and 9.1 grams of NH3 is formed, how many grams of HCI must simultaneously be formed? | grams HCl
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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![### Decomposition of NH₄Cl
The compound **NH₄Cl** can be decomposed to form **NH₃** and **HCl**. This decomposition can be represented at the atomic level by the following chemical equation:
\[ \text{NH}_4\text{Cl} \rightarrow \text{NH}_3 + \text{HCl} \]
#### Law of Conservation of Mass Application
According to the law of conservation of mass, the mass of the reactants must equal the mass of the products in a chemical reaction. If **28.5 grams** of **NH₄Cl** decomposes and results in the formation of **9.1 grams** of **NH₃**, we need to determine the mass of **HCl** that must simultaneously be formed.
\[ \text{Mass of NH₄Cl} = \text{Mass of NH₃} + \text{Mass of HCl} \]
Given:
- Mass of NH₄Cl = 28.5 grams
- Mass of NH₃ = 9.1 grams
To find:
- Mass of HCl = ? grams
Using the conservation of mass:
\[ 28.5 \, \text{grams} = 9.1 \, \text{grams} + \text{Mass of HCl} \]
Solving for the mass of HCl:
\[ \text{Mass of HCl} = 28.5 \, \text{grams} - 9.1 \, \text{grams} \]
\[ \text{Mass of HCl} = 19.4 \, \text{grams} \]
Therefore, **19.4 grams of HCl** must be formed.
**Input Field for Mass of HCl Calculation:**
\[ \boxed{19.4} \, \text{grams HCl} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1f61489d-b599-4717-b8e4-1c0e8dbf11ad%2Ff0966871-c179-4a0d-92ed-fda711bb134d%2Ff4v2fci.png&w=3840&q=75)
Transcribed Image Text:### Decomposition of NH₄Cl
The compound **NH₄Cl** can be decomposed to form **NH₃** and **HCl**. This decomposition can be represented at the atomic level by the following chemical equation:
\[ \text{NH}_4\text{Cl} \rightarrow \text{NH}_3 + \text{HCl} \]
#### Law of Conservation of Mass Application
According to the law of conservation of mass, the mass of the reactants must equal the mass of the products in a chemical reaction. If **28.5 grams** of **NH₄Cl** decomposes and results in the formation of **9.1 grams** of **NH₃**, we need to determine the mass of **HCl** that must simultaneously be formed.
\[ \text{Mass of NH₄Cl} = \text{Mass of NH₃} + \text{Mass of HCl} \]
Given:
- Mass of NH₄Cl = 28.5 grams
- Mass of NH₃ = 9.1 grams
To find:
- Mass of HCl = ? grams
Using the conservation of mass:
\[ 28.5 \, \text{grams} = 9.1 \, \text{grams} + \text{Mass of HCl} \]
Solving for the mass of HCl:
\[ \text{Mass of HCl} = 28.5 \, \text{grams} - 9.1 \, \text{grams} \]
\[ \text{Mass of HCl} = 19.4 \, \text{grams} \]
Therefore, **19.4 grams of HCl** must be formed.
**Input Field for Mass of HCl Calculation:**
\[ \boxed{19.4} \, \text{grams HCl} \]
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