Use the following information to answer questions 14-16 The radius of atoms and ions is typically measured in Angstroms \((A),\) which is equivalent to \(1 * 10^{-10} \mathrm{m} .\) Below is a table of information for three different elements. TABLE NOT AVAILABLE Neon has a smaller atomic radius than phosphorus because: (A) Unlike neon, phosphorus has electrons present in its third energy level. (B) Phosphorus has more protons than neon, which increases the repulsive forces in the atom. (C) The electrons in a neon atom are all found in a single energy level. (D) Phosphorus can form anions, while neon is unable to form any ions.

Short Answer

Expert verified
The correct answer is (D). A catalyst lowers the activation energy of the overall reaction and speeds it up.

Step by step solution

01

Understanding the Role of Catalyst

The first step is to understand the role of a catalyst in a chemical reaction. A catalyst is a substance that changes the rate or speed of a chemical reaction without being consumed by the reaction.
02

Identifying the Appropriate Choice

The next step is to identify which of the options accurately represent the role of a catalyst in a reaction. (A) Is incorrect because catalysts are not necessary for all decomposition reactions to occur. (B) Is incorrect because catalysts don't reduce the bond energy in the reactants, they provide a different pathway for the reaction with a lower activation energy. (C) Is also incorrect because catalysts don't reduce the energy differential between the reactants and products, they just lower the energy needed to get the reaction started. (D) correctly states that a catalyst lowers the activation energy of the overall reaction, making the reaction occur faster.

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Key Concepts

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

Chemical Kinetics
Understanding the concept of chemical kinetics is essential when examining how a catalyst affects a chemical reaction. Chemical kinetics is the study of the rates at which chemical processes occur and the factors that influence these rates. It includes the analysis of how different conditions can affect the speed of a reaction, such as temperature, concentration of reactants, surface area, and the presence of a catalyst.

When a catalyst is introduced into a reaction, like the decomposition of potassium chlorate mentioned in the exercise, it speeds up the reaction without being consumed. It achieves this by offering an alternative pathway for the reaction with a lower activation energy. As the kinetics of the reaction are altered, educators and students can observe the rate enhancements and gain a more profound comprehension of the mechanism by which catalysts operate.
Activation Energy
The term activation energy refers to the minimum amount of energy required for reactants to transform into products in a chemical reaction. It is a key concept in both chemistry and the process of catalysis. The activation energy serves as an energy barrier that must be overcome for a chemical reaction to proceed.

As demonstrated in the exercise, a catalyst's role is to lower this energy barrier, effectively making it easier for reactant particles to collide with enough energy to react. A reduced activation energy means that more particles have sufficient energy to undergo the reaction at a given temperature, thus increasing the reaction rate. It's important when preparing for exams like AP Chemistry to understand that activation energy can be visualized on an energy profile diagram where the effect of a catalyst appears as a lower 'hump' along the reaction path.
Decomposition Reactions
In decomposition reactions, a single compound breaks down into two or more simpler substances. These reactions are part of the foundational concepts in chemistry and often involve the breakdown of a compound when heated, as seen in the exercise with potassium chlorate. Identifying and predicting the products of decomposition reactions requires an understanding of chemical bonds and the conditions that cause them to break.

The involvement of a catalyst in this type of reaction, as in our exercise, does not change the products or the thermodynamics of the reaction. Instead, it provides a pathway for the reaction to proceed more readily by lowering the activation energy, which enhances the learning of energy concepts and reaction dynamics for students tackling AP Chemistry topics. It's essential to grasp that not all decomposition reactions require a catalyst but using one can significantly speed up the process.
AP Chemistry Exam Preparation
For students preparing for the AP Chemistry exam, mastering the role of a catalyst in chemical reactions is critical. The exam tests understanding of chemical principles and the ability to apply these principles in real-world scenarios.

Preparation should include practicing problems like the decomposition of potassium chlorate and understanding the theoretical underpinnings, such as chemical kinetics and activation energy. It should also involve familiarization with varied types of reactions, including decomposition, and being able to discern why choices like (B) or (C) in our exercise are incorrect explanations of catalyst function. High-quality exam preparation combines the development of problem-solving skills with a deep theoretical understanding of key concepts. As an exam tip, remember to approach multiple-choice questions by methodically eliminating the incorrect options, as was done in the step-by-step solution, to arrive at the correct answer efficiently.

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Most popular questions from this chapter

\(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+6 \mathrm{I}^{-}+14 \mathrm{H}^{+} \rightarrow 2 \mathrm{Cr}^{3+}+3 \mathrm{I}_{2}+7 \mathrm{H}_{2} \mathrm{O}\) Which of the following statements about the reaction given above is NOT true? (A) The oxidation number of chromium changes from \(+6\) to \(+3 .\) (B) The oxidation number of iodine changes from \(-1\) to 0. (C) The oxidation number of hydrogen changes from +1 to 0. (D) The oxidation number of oxygen remains the same.

How many liters of distilled water must be added to 1 liter of an aqueous solution of HCl with a pH of 1 to create a solution with a pH of 2? (A) 0.1 L (B) 0.9 L (C) 2 L (D) 9 L

Starting with a stock solution of 18.0 \(\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) , what is the proper procedure to create a 1.00 \(\mathrm{L}\) sample of a 3.0 \(\mathrm{M}\) solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in a volumetric flask? (A) Add 167 mL of the stock solution to the flask, then fill the flask the rest of the way with distilled water while swirling the solution. (B) Add 600 mL of the stock solution to the flask, then fill the flask the rest of the way with distilled water while swirling the solution. (C) Fill the flask partway with water, then add 167 mL of the stock solution, swirling to mix it. Last, fill the flask the rest of the way with distilled water. (D) Fill the flask partway with water, then add 600 mL of the stock solution, swirling to mix it. Last, fill the flask the rest of the way with distilled water.

$$2 \mathrm{NOCl} \rightarrow 2 \mathrm{NO}+\mathrm{Cl}_{2}$$ The reaction above takes place with all of the reactants and products in the gaseous phase. Which of the following is true of the relative rates of disappearance of the reactants and appearance of the products? (A) NO appears at twice the rate that NOCl disappears. (B) NO appears at the same rate that NOCl disappears. (C) NO appears at half the rate that NOCl disappears. (D) \(\mathrm{Cl}_{2}\) appears at the same rate that NOCl disappears.

A gas sample with a mass of 10 grams occupies 5.0 liters and exerts a pressure of 2.0 atm at a temperature of \(26^{\circ} \mathrm{C} .\) Which of the following expressions is equal to the molecular mass of the gas? The gas constant, \(R,\) is \(0.08(\mathrm{L} \times \mathrm{atm}) / \mathrm{mol} \times \mathrm{K}\) ). (A) \((0.08)(299) \mathrm{g} / \mathrm{mol}\) (B) \(\frac{(299)(0.50)}{(2.0)(0.08)} \mathrm{g} / \mathrm{mol}\) (C) \(\frac{299}{0.08} \mathrm{g} / \mathrm{mol}\) (D) \((2.0)(0.08) \mathrm{g} / \mathrm{mol}\)

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