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Chapter 6: Problem 15

State the law of mass action.

Short Answer

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Question: State the law of mass action and define the terms involved in the general form of the law. Answer: The law of mass action states that the rate of a chemical reaction is proportional to the product of the concentrations of the reactants, each raised to a power equal to the stoichiometric coefficient in the balanced chemical equation. The terms involved in the general form are: 1. Reaction Rate: The speed at which a chemical reaction proceeds. 2. Concentration: The amount of substance (moles) per unit volume (usually specified in moles per liter). 3. Stoichiometric Coefficient: The number in front of a chemical species in a balanced chemical equation that indicates the ratio in which the species reacts or is produced.

Step by step solution

01

1. Stating the general form of the law of mass action

The law of mass action states that the rate of a chemical reaction is proportional to the product of the concentrations of the reactants, each raised to a power equal to the stoichiometric coefficient in the balanced chemical equation.
02

2. Define the terms involved

- Reaction Rate: The speed at which a chemical reaction proceeds. - Concentration: The amount of substance (moles) per unit volume (usually specified in moles per liter). - Stoichiometric Coefficient: The number in front of a chemical species in a balanced chemical equation that indicates the ratio in which the species reacts or is produced.
03

3. Expressing the law of mass action using a chemical reaction example

Let's consider a generic chemical reaction as follows: aA + bB <=> cC + dD where A and B are reactants, C and D are products, and a, b, c, and d are their respective stoichiometric coefficients. According to the law of mass action, the forward reaction rate (R1) and reverse reaction rate (R2) can be described as: R1 = k1[A]^a[B]^b R2 = k2[C]^c[D]^d where [A], [B], [C], and [D] are the concentrations of each species, and k1 and k2 are the rate constants for the forward and reverse reactions, respectively. At equilibrium, both forward and reverse reaction rates are equal (R1 = R2). Thus, we can use the law of mass action to find the equilibrium constant (K_eq) for the reaction, which is given by: K_eq = (k1/k2) = ([C]^c[D]^d)/([A]^a[B]^b) This equation describes how the concentration of reactants and products relate to one another at equilibrium according to the law of mass action.

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Key Concepts

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

Reaction Rate
The reaction rate is a fundamental concept in chemistry, indicating how fast or slow a chemical reaction occurs. It essentially measures the speed at which reactants are converted into products. Understanding reaction rates helps us control how efficiently substances are transformed in industrial processes and biological systems.
For example, if we have a reaction where substance A is converted to substance B, the reaction rate would tell us how quickly A turns into B over a specific period. Factors like temperature, pressure, and catalysts can influence the reaction rate, often increasing or decreasing the speed to achieve a desired outcome.
Chemical Reaction
A chemical reaction involves the transformation of one or more substances into new products. This process is governed by the rearrangement of atoms and is described by a balanced chemical equation.
Each chemical reaction features reactants, the starting materials, and products, the substances formed as a result of the reaction. For instance, in a simple reaction:
  • H2 + O2 鈫� H2O
The reactants, hydrogen and oxygen, react to form water, which is the product.
Understanding chemical reactions is pivotal in fields ranging from pharmacology to environmental science, as it helps predict the outcomes and manage the conditions required for desired reactions.
Concentration
Concentration refers to the amount of a substance present in a certain volume of a solution, typically expressed in moles per liter (M). It's a crucial factor in the law of mass action, as the rate of a reaction depends on the concentration of the reactants.
When solutions are more concentrated, there are more reactant molecules available to interact, generally leading to a faster reaction rate. Conversely, a diluted solution tends to react more slowly.
For instance, if we have a solution where reactant A has a concentration of 2 M, it suggests that there are 2 moles of A per liter, impacting how quickly A can form products in a given chemical reaction.
Stoichiometric Coefficient
The stoichiometric coefficient is a number written before a reactant or product in a chemical equation. It indicates the proportion in which substances participate in the reaction. Think of it as a recipe: it tells you how much of each ingredient you need to achieve the desired dish鈥攐r chemical product.
For example, in the equation:
  • 2H2 + O2 鈫� 2H2O
The coefficients 2 and 1 before H2 and O2 show that two moles of hydrogen react with one mole of oxygen to produce two moles of water. This ratio is necessary to maintain a balanced equation, ensuring matter is conserved during the reaction.
Equilibrium Constant
The equilibrium constant, denoted as \( K_{eq} \), is a mathematical value that describes the ratio of products to reactants when a chemical reaction has reached equilibrium. At this point, the forward and reverse reactions occur at the same rate, meaning the concentration of reactants and products remains constant over time.
The formula for the equilibrium constant in a generic reaction
  • aA + bB 鈫� cC + dD
is given by:
\[K_{eq} = \frac{[C]^c[D]^d}{[A]^a[B]^b}\]
This equation illustrates how the concentrations of products (C and D) over the reactants (A and B), raised to their stoichiometric coefficients, are used to determine \( K_{eq} \). This helps chemists predict whether a reaction favors the formation of products or reactants under a given set of conditions.

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Most popular questions from this chapter

Explain the effect of temperature on rate of reaction on the basis of collision theory.

State and explain the law of mass action. Apply it to the following equilibria. (i) \(\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}\) (ii) \(\mathrm{NH}_{4} \mathrm{HS}_{(\mathrm{S})} \rightleftharpoons \mathrm{NH}_{3_{(\mathrm{g})}}+\mathrm{H}_{2} \mathrm{~S}_{(\mathrm{g})}\) (iii) \(2 \mathrm{SO}_{2_{(\mathrm{g})}}+\mathrm{O}_{2_{(\mathrm{g})}} \rightleftharpoons 2 \mathrm{SO}_{ \left.3_{(\mathrm{g}}\right)}\)

Explain the dynamic nature of chemical equilibrium.

Rusting of iron is a _____ reaction.

State and explain the postulates of the collision theory of reaction rates.
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