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Chapter 16: Problem 72

Why does an increase in temperature favor an increase in the speed of a reaction?

Short Answer

Expert verified
An increase in temperature favors an increase in the speed of a reaction because it raises the average kinetic energy of particles. As the temperature increases, particles move faster and collide more energetically, increasing the probability of overcoming the activation energy barrier and successful collisions that form products.

Step by step solution

01

Understand reaction rates

Reaction rates refer to the speed at which a chemical reaction occurs. This is typically measured as the change in the concentration of reactants or products over a specific period. There are several factors that can influence the rate of a reaction, including temperature, concentration, surface area, and the addition of catalysts.
02

Examine the role of kinetic energy in chemical reactions

In chemical reactions, molecules or atoms collide with one another, forming and breaking bonds to create new products. The kinetic energy of these particles plays a crucial role in determining the likelihood of successful collisions. Greater kinetic energy implies more intense collisions, increasing the chances of bond formation or breakage processes.
03

Relate temperature to kinetic energy

Temperature is a measure of the average kinetic energy of the particles in a system. When the temperature increases, the average kinetic energy of the particles also increases. This means that the particles are moving faster, and their collisions will be more energetic.
04

Understand the activation energy

For a reaction to occur, the particles involved need to overcome a specific energy barrier called activation energy (E_a). Activation energy is the minimum energy required for the reactants to form products in a chemical reaction. If the particles have sufficient energy to overcome the activation energy barrier, the reaction can proceed.
05

Apply the effect of temperature on reaction rate

With an increase in temperature, the kinetic energy of particles increases, and there is a greater probability that more particles have the necessary energy to surpass the activation energy barrier. This results in a higher frequency of successful collisions between reacting particles that form products, ultimately increasing the reaction rate. In conclusion, an increase in temperature favors an increase in the speed of a chemical reaction because it raises the average kinetic energy of particles, making it more likely for them to have sufficient energy to overcome the activation energy barrier and leading to more successful collisions that form products.

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Most popular questions from this chapter

What is the effect on the equilibrium position if an endothermic reaction is performed at a higher temperature? Does the net amount of product increase or decrease? Does the value of the equilibrium constant change if the temperature is increased?

Suppose a reaction has the equilibrium constant \(K=\) \(1.3 \times 10^{8} .\) What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?

Write the equilibrium expression for each of the following reactions. a. \(2 \mathrm{O}_{3}(g) \rightleftharpoons 3 \mathrm{O}_{2}(g)\) b. \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) c. \(C_{2} H_{4}(g)+C l_{2}(g) \rightleftharpoons C_{2} H_{4} C l_{2}(g)\).

Suppose the reaction system $$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$$ has already reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. Additional oxygen is injected into the system. b. \(\mathrm{NO}_{2}\) is removed from the reaction vessel. c. 1.0 mol of helium is injected into the system.

Write the equilibrium expression for each of the following heterogeneous equilibria. a. \(\mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{P}_{4} \mathrm{O}_{10}(s)\) b. \(\mathrm{CO}_{2}(g)+2 \mathrm{NaOH}(s) \rightleftharpoons \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)\) c. \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\).
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