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Chapter 3: Problem 73

(a) Define the terms limiting reactant and excess reactant. (b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant? (c) Why should you base your choice of which compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

Short Answer

Expert verified
The limiting reactant is used up first, determining product amounts. It's based on moles because reactions depend on molecule counts, not mass.

Step by step solution

01

Defining Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction and thus determines the maximum amount of product that can be formed. Once this reactant is exhausted, the reaction stops.
02

Defining Excess Reactant

The excess reactant is the substance that remains after the limiting reactant is completely consumed. This reactant is present in a quantity greater than necessary to react with the limiting reactant.
03

Role of Limiting Reactant

The amounts of products formed are determined by the limiting reactant because it is the reactant that is fully consumed. According to the stoichiometry of the reaction, the limiting reactant restricts the formation of products as no more product can be formed once it is depleted.
04

Why Moles Matter

The choice of the limiting reactant should be based on the number of initial moles rather than initial mass because chemical reactions occur at the molecular or atomic level. Moles represent the actual number of molecules or atoms, which directly relates to the balanced chemical equation, while mass only gives the total weight without regard to the stoichiometric relationship.

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Key Concepts

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

Excess Reactant
In many chemical reactions, you'll find that not all reactants are consumed completely. The reactant that remains after the chemical reaction has completed is known as the excess reactant. This happens because reactions often involve techniques where one reactant is left over once the limiting reactant is fully consumed.
The key reason some reactants are left in surplus is usually due to how they were mixed or because the reactant quantities weren't perfectly balanced to react entirely with each other.
  • The excess reactant has more moles available than necessary for the reaction.
  • It isn't completely used up when the reaction stops.
It's often useful to identify the excess reactant when planning reactions to optimize the usage of materials or in industrial processes.
Stoichiometry
Stoichiometry is like following a recipe in cooking. Just as recipes require specific ingredient amounts to make the desired dish, stoichiometry involves using balanced chemical equations to determine the right proportions of reactants and products in a chemical reaction.
In practical terms, stoichiometry is used to calculate the amounts of reactants needed, and therefore the quantities of products that are formed.
  • Relies on a balanced chemical equation.
  • Helps determine the limiting reactant, which is fully consumed.
  • Ensures chemical reactions are efficient and predictable.
By understanding stoichiometry, students and scientists can predict how much of each substance will be used or produced in a given reaction.
Chemical Reactions
Chemical reactions occur when substances interact to form new products, and they are fundamental to chemistry. These reactions involve breaking and forming chemical bonds between atoms.
When learning about chemical reactions, several core ideas are vital to grasp:
  • Chemical equations balance the number of atoms of each element on both sides.
  • Atoms rearrange but are not lost or gained in reactions.
  • In any reaction, the identity of reactants and products, along with their amounts, matter greatly.
Understanding these concepts helps clarify why certain products form and how different conditions can affect the reaction's outcome.
Moles in Chemistry
The concept of moles is central to quantifying substances in chemistry. A mole refers to a quantity (6.022 脳 10^23) of atoms, molecules, or ions, allowing chemists to count particles by weighing a sample.
This is crucial because reactions happen at the particle level. So, measuring substances by moles rather than by mass makes it easier to relate quantities directly to chemical equations.
  • Moles allow for precise calculations in stoichiometry.
  • They relate the macroscopic world of grams to the microscopic world of atoms and molecules.
  • This enables better predictions about how substances in reactions interact and change forms.
Learning to work with moles is essential for developing a deep understanding of how reactions and compounds behave.

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Most popular questions from this chapter

A sample of the male sex hormone testosterone, \(\mathrm{C}_{19} \mathrm{H}_{28} \mathrm{O}_{2}\), contains \(3.88 \times 10^{21}\) hydrogen atoms. (a) How many atoms of carbon does it contain? (b) How many molecules of testosterone does it contain? (c) How many moles of testosterone does it contain? (d) What is the mass of this sample in grams?

Balance the following equations: (a) \(\mathrm{SiCl}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Si}(\mathrm{OH})_{4}(s)+\mathrm{HCl}(a q)\) (b) \(\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+\mathrm{O}_{2}(g)\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(l) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) (d) \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \longrightarrow \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

Without doing any detailed calculations (but using a periodic table to give atomic weights), rank the following samples in order of increasing numbers of atoms: \(0.5 \mathrm{~mol} \mathrm{BCl}_{3}\) molecules, \(197 \mathrm{~g}\) gold, \(6.0 \times 10^{23} \mathrm{CCl}_{4}\) molecules.

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write the balanced chemical equation for this reaction. (b) How many grams of aluminum hydroxide are obtained from \(14.2 \mathrm{~g}\) of aluminum sulfide?

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If \(5.00 \mathrm{~g}\) of sulfuric acid and \(5.00 \mathrm{~g}\) of lead(II) acetate are mixed, calculate the number of grams of sulfuric acid, lead(II) acetate, lead(II) sulfate, and acetic acid present in the mixture after the reaction is complete.
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