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Chapter 7: Problem 176

(A): A catalyst enhances the rate of reaction. (R) : The energy of activation of the reaction is lowered in presence of a catalyst.

Short Answer

Expert verified
Both (A) and (R) are correct, and (R) is the correct explanation of (A).

Step by step solution

01

Understanding Statement (A)

Statement (A) claims that a catalyst enhances the rate of a reaction. Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. By definition, a catalyst speeds up the reaction by providing an alternative reaction pathway.
02

Understanding Statement (R)

Statement (R) proposes that the energy of activation is lowered in the presence of a catalyst. The energy of activation is the minimum energy required for a chemical reaction to occur. Catalysts lower this threshold, allowing the reaction to proceed more quickly because more molecules possess the necessary energy to react at a given temperature.
03

Determining the Relationship

To determine the relationship between (A) and (R), consider whether (R) explains (A). A catalyst increases the rate of a chemical reaction primarily because it lowers the activation energy (as stated in (R)). Therefore, (R) provides the reason for why (A) occurs.

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Key Concepts

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

Understanding Activation Energy
Activation energy is like the initial push you need to start a snowball rolling down a hill. It is the minimum energy required for a chemical reaction to begin.
Reactions need this push because the molecules must collide with enough force to break bonds and form new ones. Without sufficient energy, molecules just bounce off each other without reacting. This energy barrier ensures that reactions only occur when conditions are favorable, which is important for the control and stability in chemical systems. When a catalyst is added, this crucial energy threshold is lowered. This means that more molecules have enough energy to overcome it and react, which speeds up the reaction. A lower activation energy means that even at lower temperatures, reactions can occur more swiftly.
Reaction Rate and its Importance
The reaction rate is a measure of how fast a chemical reaction occurs. There are several factors that influence reaction rates, including the concentration of reactants, temperature, surface area, and the presence of a catalyst. A catalyst can dramatically increase the reaction rate by lowering the activation energy. With a catalyst, reactions that would take years can occur in a matter of seconds. This is especially critical in industrial processes, where efficiency and speed are paramount. To understand how quickly a reaction proceeds, we observe changes like color shifts or gas production, which indicate the progression of the reaction. By monitoring these changes, we can determine if a reaction is proceeding as desired and make necessary adjustments.
Basics of a Chemical Reaction
A chemical reaction involves the breaking and forming of bonds between atoms to transform substances into new products.
The reactants are the starting materials, and the products are the substances generated from the reaction. Chemical reactions are all around us, from the process of digestion converting food into energy, to plants performing photosynthesis. Reactions are governed by the Law of Conservation of Mass, which states that matter is neither created nor destroyed in a chemical reaction. This means the mass of the reactants equals the mass of the products, ensuring that atoms are simply rearranged to create new substances. Catalysts are like helpers in these reactions, facilitating the transformation by making it easier and faster, all while remaining unchanged. Understanding these principles helps one navigate the complex world of chemistry with more ease.

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Most popular questions from this chapter

For a first order reaction, which is/are correct here? a. The time taken for the completion of \(75 \%\) reaction is twice the \(t_{1 / 2}\) of the reaction b. The degree of dissociation is equal to \(1-\mathrm{e}^{-k t}\). c. A plot of reciprocal concentration of the reactant versus time gives a straight line d. The pre-exponential factor in the Arrhenius equation has the dimension of time, \(T^{-1}\).

For a first order reaction, which of the following are not correct? a. \(t_{7 / 8}=2 t_{34}\) b. \(t_{3 / 4}=2 t_{1 / 2}\) c. \(t_{15 / 16}=4 t_{1 / 2}\) d. \(t_{15 / 6}=3 t_{3 / 4}\)

The following set of data was obtained by the method of initial rates for the reaction: \(2 \mathrm{HgCl}_{2}(\mathrm{aq})+\mathrm{C}_{2} \mathrm{O}_{4}^{2-}(\mathrm{aq}) \rightarrow\) \(2 \mathrm{Cl}^{-}(\mathrm{aq})+2 \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{Hg}_{2} \mathrm{Cl}_{2}(\mathrm{~s})\) \begin{tabular}{lll} \hline\(\left[\mathrm{HgCl}_{2}\right], \mathrm{M}\) & {\(\left[\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right], \mathrm{M}\)} & Rate, \(\mathrm{M} / \mathrm{s}\) \\ \hline \(0.10\) & \(0.10\) & \(1.3 \times 10^{-7}\) \\ \(0.10\) & \(0.20\) & \(5.2 \times 10^{-7}\) \\ \(0.20\) & \(0.20\) & \(1.0 \times 10^{-6}\) \\ \hline \end{tabular} What is the value of the rate constant, \(\mathrm{k}\) ? a. \(1.6 \times 10^{-4} 1 / \mathrm{M}^{2} \cdot \mathrm{s}\) b. \(1.3 \times 10^{-4} 1 / \mathrm{M}^{2} \cdot \mathrm{s}\) c. \(1.4 \times 10^{-7} 1 / \mathrm{M}^{2} \cdot \mathrm{s}\) d. \(1.3 \times 10^{-6} 1 / \mathrm{M}^{2} \cdot \mathrm{s}\)

Two reactions \(\mathrm{X} \rightarrow\) Products and \(\mathrm{Y} \rightarrow\) products have rate constant \(k_{x}\) and \(k_{y}\) at temperature \(T\) and activation energies \(E_{x}\) and \(E_{Y}\) respectively. If \(k_{x}>\) \(\mathrm{k}_{\mathrm{r}}\) and \(\mathrm{E}_{\mathrm{x}}<\mathrm{E}_{\mathrm{Y}}\) and assuming that for both the reaction is same, then a. At lower temperature \(\mathrm{k}_{\mathrm{Y}}>\mathrm{k}_{\mathrm{x}}\) b. At higher temperature \(\mathrm{k}_{\mathrm{x}}\) will be greater than \(\mathrm{k}_{\mathrm{y}}\)c. At lower temperature \(k_{x}\) and \(k_{y}\) will be close to each other in magnitude d. At temperature rises, \(\mathrm{k}_{\mathrm{x}}\) and \(\mathrm{k}_{\mathrm{y}}\) will be close to each other in magnitude

The first order isomerisation reaction: Cyclopropane \(\rightarrow\) propene, has a rate constant of \(1.10 \times 10^{-4} \mathrm{~s}^{-1}\) at \(470^{\circ} \mathrm{C}\) and an activation energy of \(264 \mathrm{~kJ} / \mathrm{mol}\). What is the temperature of the reaction when the rate constant is equal to \(4.36 \times 10^{-3} \mathrm{~s}^{-1}\) ? a. \(240^{\circ} \mathrm{C}\) b. \(150^{\circ} \mathrm{C}\) c. \(540^{\circ} \mathrm{C}\) d. \(450^{\circ} \mathrm{C}\)
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