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Ch.3 - Chemical Reactions and Reaction Stoichiometry
All textbooksBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblem 7d2
Chapter 3, Problem 7d2

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (d) If so, how many of which type are left over?
How many N2 molecules are left over?

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1
Identify the balanced chemical equation for the reaction: \( N_2 + 3H_2 \rightarrow 2NH_3 \).
Determine the initial number of \( N_2 \) and \( H_2 \) molecules from the diagram.
Calculate the limiting reactant by comparing the mole ratio of \( N_2 \) to \( H_2 \) with the stoichiometric ratio from the balanced equation.
Use the limiting reactant to determine how many \( N_2 \) molecules are consumed in the reaction.
Subtract the number of \( N_2 \) molecules consumed from the initial number to find how many \( N_2 \) molecules are left over.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate how much of each substance is consumed or produced based on balanced chemical equations. In this case, understanding the stoichiometric ratios of nitrogen and hydrogen in the formation of ammonia is essential to determine how many molecules remain after the reaction.
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Stoichiometry Concept

Molecular Representation

Molecular representation involves visualizing molecules using symbols or models to understand their composition and structure. In the given question, nitrogen (N2) is represented by blue spheres and hydrogen (H2) by white spheres. This representation helps in identifying how many molecules of each reactant are present and how they interact during the reaction to form ammonia (NH3).
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Molecular Polarity

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating how many molecules of the other reactants remain after the reaction. In this scenario, knowing which reactant (N2 or H2) limits the formation of ammonia will help answer how many N2 molecules are left over.
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Related Practice
Textbook Question

The following diagram represents a high-temperature reaction between CH4 and H2O. Based on this reaction, find how many moles of each product can be obtained starting with 4.0 mol CH4.

Based on this reaction, find how many moles of CO can be obtained starting with 4.0 mol CH4?

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Textbook Question

The following diagram represents a high-temperature reaction between CH4 and H2O. Based on this reaction, find how many moles of each product can be obtained starting with 4.0 mol CH4. Based on this reaction, how many moles of H2 can be obtained starting with 4.0 mol CH4?

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Textbook Question

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (a) Write the balanced chemical equation for the reaction.

Textbook Question

Nitrogen 1N22 and hydrogen 1H22 react to form ammonia 1NH32. Consider the mixture of N2 and H2 shown in the accompanying diagram. The blue spheres represent N, and the white ones represent H. (d) Are any reactant molecules left over, based on the diagram?

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Textbook Question

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (a) How many molecules of NO2 can be formed, assuming the reaction goes to completion?

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Textbook Question

Nitrogen monoxide and oxygen react to form nitrogen dioxide. Consider the mixture of NO and O2 shown in the accompanying diagram. The blue spheres represent N, and the red ones represent O. (c) If the actual yield of the reaction was 75% instead of 100%, how many molecules of each kind would be present after the reaction was over?