Which of the following is the reason/s why the catalysts increase the rate of a reaction: Decreasing the energy of the reactants O Increasing the fraction of reactants that has potential energy higher than the activation energy Decreasing the energy of the transition state Increasing the energy of the transition state Increasing the kinetic energy of the reactants Decreasing the activation energy for the reaction O Increasing the fraction of reactants that has kinetic energy higher than the activation energy

Which of the following is the reason/s why the catalysts increase the rate of a reaction: Decreasing the energy of the reactants O Increasing the fraction of reactants that has potential energy higher than the activation energy Decreasing the energy of the transition state Increasing the energy of the transition state Increasing the kinetic energy of the reactants Decreasing the activation energy for the reaction O Increasing the fraction of reactants that has kinetic energy higher than the activation energy

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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How does collision orientation affect the rate of a reaction
Generally, increasing the temperature increases the rate of a reaction. This is because: O increasing the temperature increases the frequency of collisions O increasing the temperature increases the average energy of the collisions and increases the frequency of collisions O increasing the temperature lowers the activation energy of the reaction increasing the temperature increases the average energy of the collisions.
Which of the following statements is false. Catalysts make a reaction rate go faster by providing a different route for the same reaction to proceed that requires less input energy. Increasing the concentration increases the rate of a reaction because more molecules are available in the same amount of space leading to more collisions with the correct orientation. Adding energy increases the rate of a reaction because more collisions happen with enough energy to break the bonds. Increasing the pressure by adding an inert gas increases the rate of reaction by causing more collisions.
A catalyst affects the rate of the forward reaction by changing which of the following? Heat of reaction, Potential energy of the products . Heat of formation, or Activation energy
What does it mean for a reaction to release energy? The relative potential energy of the reaction is negative. The activation energy of the reaction is positive. The relative potential energy of the reaction is positive. The activation energy of the reaction is negative.
Which of the following will lower the activation energy for a reaction? Group of answer choices raising the temperature of the reaction. increasing the concentrations of reactants. increasing the surface area of the reactants. adding a suitable catalyst.
Catalysts speed up the rate of a reaction by increasing the activation energy Select one: O True O False
Which of these changes would increase the rate of a reaction? Decrease concentration Use solid rather than a gaseous form Add catalyst Decrease temperature
What is the difference between exergonic and exothermic? What is the difference between intermediate and transition state? What is the relation between activation energy and the rate of a reaction?
Which of the following is true? Decreasing the activation energy decreases the reaction rate. Decreasing the activation energy increases the reaction rate. The activation energy of an exothermic reaction is negative. There is no relationship between activation energy and reaction rate.