   # “Smelling salts,” which are used to revive someone who has fainted, typically contain ammonium carbonate, ( NH 4 ) 2 CO 3 . Ammonium carbonate decomposes readily to form ammonia, carbon dioxide, and water. The strong odor of the ammonia usually restores consciousness in the person who has tainted. The unbalanced equation is :math&gt; ( NH 4 ) 2 CO 3 ( s ) → NH 3 ( g ) + CO 2 ( g ) + H 2 O ( g ) lculate the mass of ammonia gas that is produced if 1 .25 g of ammonium carbonate decomposes completely. ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425
Chapter 9, Problem 27QAP
Textbook Problem
425 views

## “Smelling salts,” which are used to revive someone who has fainted, typically contain ammonium carbonate, ( NH 4 ) 2 CO 3 . Ammonium carbonate decomposes readily to form ammonia, carbon dioxide, and water. The strong odor of the ammonia usually restores consciousness in the person who has tainted. The unbalanced equation is:math> ( NH 4 ) 2 CO 3 ( s ) → NH 3 ( g ) + CO 2 ( g ) + H 2 O ( g ) lculate the mass of ammonia gas that is produced if 1 .25 g of ammonium carbonate decomposes completely.

Interpretation Introduction

Interpretation:

The mass of ammonia produced should be calculated.

Concept Introduction:

The decomposition of ammonium carbonate gives ammonia and carbon dioxide as follows:

(NH4)2CO3(s)NH3(g)+CO2(g)+H2O(g)

For complete decomposition reaction, mass of ammonia can be calculated from its number of moles that depends on the number of moles of ammonium carbonate.

### Explanation of Solution

To calculate the mass of ammonia gas, first calculate number of moles of ammonium carbonate as follows:

n=mM

Here, m is mass and M is molar mass

Mass of ammonium carbonate is 1.25 g and molar mass is 53.5 g/mol

Putting the values,

n=1.25 g53.5 g/mol=0.0234 mol

From the balanced chemical reaction as follows:

(NH4)2CO3(s)2NH3

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