   # Consider the following reaction: 4 NH 3 ( g ) → 4 NO ( g ) + 6 H 2 O ( g ) If a container were to have 10 molecules of O 2 and 10 molecules of NH 3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 5, Problem 116E
Textbook Problem
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## Consider the following reaction: 4 NH 3 ( g ) → 4 NO ( g )   +   6 H 2 O ( g ) If a container were to have 10 molecules of O2 and 10 molecules of NH3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?

Interpretation Introduction

Interpretation: The total number of reactant and product molecules present in the given container after the completion of the reaction is to be calculated.

Concept introduction: According to the law of conservation of mass, mass can neither be created nor destroyed. The mass of reactants is equal to the mass of products formed during a chemical process.

To determine: The total number of molecules present after the completion of the stated chemical reaction.

### Explanation of Solution

Given

The stated chemical reaction is,

4NH3(g)+5O2(g)4NO(g)+6H2O(g)

5mol of O2 react with 4mol of NH3 .

1mol of O2 reacts with NH3 =(45)mol

10mol of O2 reacts with NH3 =(4×105)mol=8mol

There are 10mol of ammonia present. Hence, 2mol of ammonia will be left unreacted.

5mol of O2 produce 4mol of NO .

1mol of O2 produces NO =(45)mol

10mol of O2 produces NO =(4×105)mol=8mol

The amount of NO produced is 8mol

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