Which statement about the factors that affect reaction rates is false? Question 8 options: Decreasing the concentrations of the reacting particles decreases the chance of collision. A collision with poor orientation requires a higher activation energy than a collision with optimum orientation. Increasing the pressure in a gaseous reaction increases the chance of collision. A reaction occurs every time particles of the reactants collide. Increasing the temperature increases the reaction rate.

Option a: This option is true because the higher the concentration of the reactants, the higher the…

Answered: Which statement about the factors that…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 62A

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Apply collision theory to explain why powdered zinc reacts to form hydrogen gas faster than large pieces of zinc when both are placed in hydrochloric acid solution.
Classify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.
What happens to the reactants in an ineffective molecular collision?
Apply collision theory to explain why increasing the concentration of a reactant usually increases the reaction rate.
How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate.
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
. How does the collision model account for the fact that a react ion proceeds faster when the concentrations of the reactants are increased?
What is the role of the activated complex in a chemical reaction?
. Account for the increase in reaction rate brought about by a catalyst.
Which reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?

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	Decreasing the concentrations of the reacting particles decreases the chance of collision.
	A collision with poor orientation requires a higher activation energy than a collision with optimum orientation.
	Increasing the pressure in a gaseous reaction increases the chance of collision.
	A reaction occurs every time particles of the reactants collide.
	Increasing the temperature increases the reaction rate.