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Chapter 3: Problem 10

What is a limiting reactant in a reaction mixture? Explain how it determines the amount of product.

Short Answer

Expert verified
A limiting reactant is consumed first, determining the amount of product.

Step by step solution

01

Understanding Limiting Reactant Concept

A limiting reactant is a substance that is totally consumed when the chemical reaction is complete. The reaction cannot proceed further once this substance is used up because there is no more of it to react with the other reactants.
02

Identify the Limiting Reactant

In a chemical reaction, compare the mole ratio of the reactants used in the reaction to the mole ratio of the reactants present. The reactant that is present in the smallest stoichiometric amount compared to what is required is the limiting reactant.
03

Impact on Product Formation

The amount of product formed in a chemical reaction is determined by the limiting reactant. Since the reaction can only proceed until the limiting reactant is used up, it defines the maximum quantity of product that can be generated.
04

Calculation Example

Suppose we have 2 moles of reactant A and 3 moles of reactant B, and the balanced equation is A + 2B 鈫� C. The stoichiometric ratio requires 1 mole of A for every 2 moles of B. With the given amounts, reactant B will be the limiting reactant because it is present in sufficient quantity to fully react with only 1 mole of A. Thus, it limits the formation of product C to 1 mole.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stoichiometry
Stoichiometry is a fundamental concept in chemistry that deals with the calculation of reactants and products in a chemical reaction. It allows us to predict the amounts of substances consumed and produced in a reaction based on their balanced chemical equation.
To perform stoichiometric calculations, you need to understand the concept of a balanced equation, where the number of atoms for each element is the same on both sides. This is critical because it tells us the exact proportions in which reactants must combine to form products.
  • It is the mathematical backbone that supports our understanding of chemical reactions.
  • Stoichiometry provides the framework for identifying limiting reactants.
  • It is essential for scaling reactions in industrial processes.
Chemical Reaction
A chemical reaction involves the transformation of reactants into products. This involves breaking and forming chemical bonds, leading to new substances with different properties.
The equation that represents a chemical reaction must be balanced to reflect the conservation of mass, meaning no atoms are lost or gained, just rearranged.
  • Chemical reactions can be categorized into types such as synthesis, decomposition, or combustion.
  • Understanding chemical reactions is key to predicting the result of mixing different substances together.
  • The type of chemical reaction affects the stoichiometry and can influence which reactant becomes limiting.
Product Formation
The formation of products in a chemical reaction is directly linked to the reactants used. Specifically, the limiting reactant determines how much product can be formed.
Once the limiting reactant is entirely consumed, the reaction stops, and no additional product can be formed, no matter how much of the other reactants are left over. This places a cap on product quantity based entirely on the limiting factor.
  • Theoretical yield is computed based on the limiting reactant's quantity.
  • Understanding this is crucial for planning reactions and minimizing waste.
  • Actual yield in practice may be less due to loss and inefficiencies.
Mole Ratio
The mole ratio is a critical concept derived from the balanced chemical equation. It tells us the proportion in which reactants react and products form.
For example, in the equation \(A + 2B \rightarrow C\), the mole ratio suggests that 1 mole of \(A\) reacts with 2 moles of \(B\) to produce 1 mole of \(C\). Calculating the mole ratio is essential for stoichiometry.
  • Mole ratios ensure that reactants are mixed in the perfect proportions to minimize waste.
  • It helps in identifying the limiting reactant by comparing calculated ratios with available quantities.
  • Using mole ratios allows prediction of product yield from known reactants.

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Most popular questions from this chapter

Carbon disulfide, \(\mathrm{CS}_{2}\), is a colorless, highly flammable liquid used in the manufacture of rayon and cellophane. A sample contains \(0.0205 \mathrm{~mol} \mathrm{CS}_{2} .\) Calculate the mass of carbon disulfide in the sample.

Part 1 a. How many hydrogen and oxygen atoms are present in 1 molecule of \(\mathrm{H}_{2} \mathrm{O} ?\) b. How many moles of hydrogen and oxygen atoms are present in \(1 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}\) ? c. What are the masses of hydrogen and oxygen in \(1.0 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}\) ? d. What is the mass of \(1.0 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}\) ? Part 2: Two hypothetical ionic compounds are discovered with the chemical formulas \(\mathrm{XCl}_{2}\) and \(\mathrm{YCl}_{2}\), where \(\mathrm{X}\) and \(\mathrm{Y}\) represent symbols of the imaginary elements. Chemical analysis of the two compounds reveals that \(0.25 \mathrm{~mol} \mathrm{XCl}_{2}\) has a mass of \(100.0 \mathrm{~g}\) and \(0.50 \mathrm{~mol} \mathrm{YCl}_{2}\) has a mass of \(125.0 \mathrm{~g}\). a. What are the molar masses of \(\mathrm{XCl}_{2}\) and \(\mathrm{YCl}_{2}\) ? b. If you had \(1.0\) -mol samples of \(\mathrm{XCl}_{2}\) and \(\mathrm{YCl}_{2}\), how would the number of chloride ions compare? C. If you had \(1.0\) -mol samples of \(\mathrm{XCl}_{2}\) and \(\mathrm{YCl}_{2}\), how would the masses of elements \(\mathrm{X}\) and \(\mathrm{Y}\) compare? d. What is the mass of chloride ions present in \(1.0 \mathrm{~mol} \mathrm{XCl}_{2}\) and \(1.0 \mathrm{~mol} \mathrm{YCl}_{2} ?\) e. What are the molar masses of elements \(\mathrm{X}\) and \(\mathrm{Y}\) ? f. How many moles of \(\mathrm{X}\) ions and chloride ions would be present in a \(200.0-\mathrm{g}\) sample of \(\mathrm{XCl}_{2}\) ? g. How many grams of \(Y\) ions would be present in a \(250.0-\mathrm{g}\) sample of \(\mathrm{YCl}_{2} ?\) h. What would be the molar mass of the compound \(\mathrm{YBr}_{3}\) ? Part 3: A minute sample of \(\mathrm{AlCl}_{3}\) is analyzed for chlorine. The analysis reveals that there are 12 chloride ions present in the sample. How many aluminum ions must be present in the sample? a. What is the total mass of \(\mathrm{AlCl}_{3}\) in this sample? b. How many moles of \(\mathrm{AlCl}_{3}\) are in this sample?

Acrylic acid, used in the manufacture of acrylic plastics, has the composition \(50.0 \% \mathrm{C}, 5.6 \% \mathrm{H}\), and \(44.4 \% \mathrm{O} .\) What is its empirical formula?

Two compounds have the same composition: \(85.62 \%\) C and \(14.38 \% \mathrm{H}\). a. Obtain the empirical formula corresponding to this composition. b. One of the compounds has a molecular mass of \(28.03\) amu; the other, of \(56.06\) amu. Obtain the molecular formulas of both compounds.

Calculate the following. a. number of atoms in \(25.7 \mathrm{~g} \mathrm{Al}\) b. number of atoms in \(8.71 \mathrm{~g} \mathrm{I}_{2}\) c. number of molecules in \(14.9 \mathrm{~g} \mathrm{~N}_{2} \mathrm{O}_{5}\) d. number of formula units in \(3.31 \mathrm{~g} \mathrm{NaClO}_{4}\) e. number of \(\mathrm{Ca}^{2+}\) ions in \(4.71 \mathrm{~g} \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)
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