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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 15th Edition
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Tutti i libri di testoBrown 15th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 6b
Capitolo 3, Problema 6b

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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Step 1: Write down the balanced chemical equation for the reaction. The reaction between CH4 and H2O at high temperature is CH4 + H2O -> CO + 3H2. This equation tells us that one mole of CH4 reacts with one mole of H2O to produce one mole of CO and three moles of H2.
Step 2: Identify the given and what needs to be found. In this case, we are given that we have 4.0 mol of CH4 and we need to find out how many moles of each product can be obtained.
Step 3: Use the stoichiometry of the reaction to calculate the moles of the products. According to the balanced chemical equation, one mole of CH4 produces one mole of CO and three moles of H2. Therefore, 4.0 mol of CH4 will produce 4.0 mol of CO and 4.0*3 = 12.0 mol of H2.
Step 4: Therefore, starting with 4.0 mol CH4, we can obtain 4.0 mol CO and 12.0 mol H2.
Step 5: To answer the second part of the question, how many moles of H2 can be obtained starting with 4.0 mol CH4, we already calculated that in step 3. So, starting with 4.0 mol CH4, we can obtain 12.0 mol H2.

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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 the amount of products formed or reactants consumed based on balanced chemical equations. Understanding stoichiometry is essential for determining how many moles of products can be produced from a given amount of reactants.
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Stoichiometry Concept

Balanced Chemical Equation

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It provides the mole ratios of reactants and products, which are crucial for stoichiometric calculations. For the reaction between CH4 and H2O, knowing the balanced equation helps in determining the moles of H2 produced from a specific amount of CH4.
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Balancing Chemical Equations

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 vital for accurate stoichiometric calculations, as it dictates how much of the other reactants will remain unreacted. In this case, understanding which reactant limits the production of H2 from CH4 is key to solving the problem.
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Domanda del libro di testo

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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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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Glycine, an amino acid used by organisms to make proteins, is represented by the following molecular model. (d) Calculate the percent nitrogen by mass in glycine.

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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.

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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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