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Chapter 9: Problem 42

Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Is the mole ratio in which the reactants combine involved?

Short Answer

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To determine the limiting reactant in a chemical reaction, one must consider both the masses of the reactants present and the mole ratios in which they combine. First, calculate the amount of product that can be formed from the available amounts of each reactant by dividing the moles of each reactant by their respective coefficients in the balanced chemical equation. Then, compare the results to identify the limiting reactant - the reactant that yields the least amount of product. This reactant will be consumed first, limiting the reaction's progress.

Step by step solution

01

Review the Concept of Limiting Reactants

In a chemical reaction, the limiting reactant is the reactant that is completely consumed first and limits the extent of the reaction, determining the maximum amount of product that can be formed. Essentially, the reaction stops once the limiting reactant is used up.
02

Understand the Importance of Mole Ratios

Mole ratios refer to the ratio of moles of one reactant to the moles of another reactant involved in a chemical reaction. In a balanced chemical equation, the coefficients of the reactants represent their mole ratios. Mole ratios determine how reactants react with each other and are essential for calculating the expected amount of products formed.
03

Determine the Amount of Product Formed from Each Reactant

To determine which reactant is the limiting reactant, we first need to calculate the amount of product that can be formed from the available amounts of each reactant. To do this, divide the moles of each reactant by their respective coefficients in the balanced chemical equation. This will give the maximum amount of product that can be formed from each reactant.
04

Identify the Limiting Reactant

After calculating the maximum amount of product formed from each reactant, compare the results. The reactant that yields the least amount of product will be the limiting reactant. In other words, the limiting reactant is the reactant consumed completely in producing a smaller amount of product. In conclusion, determining the limiting reactant depends on both the masses of the reactants and the mole ratios in which they combine. By comparing the amounts of product that can be formed from each reactant's given moles and considering their mole ratios, we can determine which reactant will be consumed first and limit the reaction's progress.

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Key Concepts

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

Chemical Reaction
Every chemical reaction involves the transformation of reactants into products. To better understand this, imagine a recipe, where ingredients are the reactants and the dish is the product. A chemical reaction is an organized way of producing new substances from existing ones by rearranging atoms.
鈥� During a reaction, bonds between atoms in the reactants are broken, and new bonds are formed to create the products.
鈥� Reactions can be simple, involving just a few substances, or complex, with many reactants and products.
鈼� In practice, some reactants may not react completely, leading us to the concept of limiting reactants. This is especially crucial in understanding how much product can be formed.
In summary, a chemical reaction is the process through which new substances are formed, defined by changes in atomic bonds. Understanding this helps set the stage for figuring out potential outcomes, like the amount of product formed, and is fundamental to answering the question of limiting reactants.
Mole Ratios
Mole ratios are crucial in analyzing any chemical reaction. Simply put, a mole ratio represents the ratio between the amounts of any two substances involved in a reaction. These ratios are derived from the coefficients found in a balanced chemical equation.

For example, consider the balanced reaction:
2H鈧� + O鈧� 鈫� 2H鈧侽
Here, the mole ratio of hydrogen to oxygen is 2:1, meaning for every 2 moles of hydrogen, 1 mole of oxygen is required.
鈥� Mole ratios let us predict how reactants will react and how much of each is needed.
鈥� It also helps in determining which reactant might run out first, thus becoming the limiting reactant.
In any analysis regarding chemical reactions, proper understanding of mole ratios ensures accurate predictions about the extent of the reaction, making them pivotal in calculations involving limiting reactants.
Balanced Chemical Equation
A balanced chemical equation is more than just a way to represent a chemical reaction. It is a crucial tool that shows the exact proportions in which elements or compounds react and form products.
鈥� Balancing ensures the law of conservation of mass is upheld, meaning the mass of reactants equals the mass of products.
鈥� In balancing, coefficients are adjusted to reflect the smallest whole number ratio of reactants and products. For example, the equation for the combustion of methane:
CH鈧� + 2O鈧� 鈫� CO鈧� + 2H鈧侽
Here, balancing ensures 1 carbon, 4 hydrogen, and 4 oxygen atoms are on each side.
These coefficients are vital for calculating how much of each reactant is needed and what is produced, which is particularly important when determining the limiting reactant.
Balanced equations guide us in making accurate predictions and calculations in chemical reactions, confirming their status as science's blueprint for reaction analysis.

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Most popular questions from this chapter

Many metals occur naturally as sulfide compounds; examples include \(\mathrm{ZnS}\) and \(\mathrm{CoS}\). Air pollution often accompanies the processing of these ores, because toxic sulfur dioxide is released as the ore is converted from the sulfide to the oxide by roasting (smelting). For example, consider the unbalanced equation for the roasting reaction for zinc: $$\mathrm{ZnS}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{ZnO}(s)+\mathrm{SO}_{2}(g)$$ How many kilograms of sulfur dioxide are produced when \(1.0 \times 10^{2} \mathrm{kg}\) of \(\mathrm{ZnS}\) is roasted in excess oxygen by this process?

Using the average atomic masses given inside the front cover of this book, calculate how many moles of each substance the following masses represent. a. \(12.7 \mathrm{g}\) of hydrogen gas, \(\mathrm{H}_{2}\) b. \(5.2 \mathrm{g}\) of calcium hydride, \(\mathrm{CaH}_{2}\) c. 41.6 mg of potassium hydroxide, KOH d. \(6.93 \mathrm{g}\) of hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{S}\) e. \(94.7 \mathrm{g}\) of water, \(\mathrm{H}_{2} \mathrm{O}\) f. 321 mg of lead g. 8.79 g of silver nitrate, \(\mathrm{AgNO}_{3}\)

What do the coefficients of a balanced chemical equation tell us about the proportions in which substances react on a macroscopic (mole) basis?

Consider the unbalanced chemical equation $$\mathrm{CaH}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2}(g)$$ Balance the equation and then write the mole ratios that would allow you to calculate the number of moles of each product that would form for a given number of moles of water reacting.

The traditional method of analysis for the amount of chloride ion present in a sample was to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding a slight excess of silver nitrate, it is possible effectively to remove all chloride ion from the sample. $$ \mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{AgCl}(s) $$ Suppose a \(1.054-\mathrm{g}\) sample is known to contain \(10.3 \%\) chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample? What mass of silver chloride will be obtained?
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