Which statement could NOT be a possible explanation for the increase in effective collisions caused by a catalyst? A. The catalyst provides a surface to improve the chance of correct orientation. B. The catalyst lowers the activation energy increasing the number of reactants with KE higher than E. a C. The catalyst increases reactant speed so more particles have enough KE to overcome E. a

Which statement could NOT be a possible explanation for the increase in effective collisions caused by a catalyst? A. The catalyst provides a surface to improve the chance of correct orientation. B. The catalyst lowers the activation energy increasing the number of reactants with KE higher than E. a C. The catalyst increases reactant speed so more particles have enough KE to overcome E. a

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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Which of the following changes would most likely increase the rate of a reaction? a. increasing the size of the reactant particles b. decreasing the reaction temperature c. decreasing the concentration of a reactant d. decreasing the activation energy for the reaction
Which statement is INCORRECT with regard to kinetics? A. Each 10o C rise in temperature approximately doubles the rate of a reaction. B. The rate is expressed as the change in concentration per the change in time. C. The rate of reaction is always expressed as a positive value. D. The presence of a catalyst decreases the rate of reaction by lowering the Ea of the reaction. E. The effect that changing the concentration of a reactent has on the rate of a reaction must be determined experimentally.
Which type of equation allows one to track changes in concentration vs time? a. Rate law b. integrated rate law c Arrhenius equation d. none of the above e. all of the above
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po Energy and Matter Transition States At the peak of the Reaction Pathways graph, there is a brief interval between the time that the reactant bonds are broken and product bonds are formed. This transitional structure is called an activated complex, and it exists for only a brief period of time. Just because the activated complex forms does not necessarily mean products will form. It may return to the original reactants, Increasing the temperature of the reaction causes more particles to have sufficient energy to form the activated complex on collision. That is why reaction rate increases as temperature increases. Increasing temperature increases the opportunities for products to form. APPLY How does concentration affect the formation of the activated complex? Haughton Miflin Harcourt Publishing Company
6. The rate constants for the decomposition of a compound are 6.2 x 10* s' at 45°C and 2.1 x 103 s1 at 55°C. What is the value of the activation energy for this reaction in kJ/mol? А. 1.7 х 10% В. 1.1 x 105 C. 2.5 x 103 D. 2.5 x 104 E. 1.1x 106
Each step represents an elementary reaction. Step1. A + 2B + C (fast equilibrium, k and k.j) Step2. C +D → E (slow, k2) a. Find the balanced equation. *b. Order the species as 'Catalyst', 'Intermediate', 'Reactant' or 'Product'. *c. Find the rate-determining step (RDS) and express the rate law. d. Use the Pre-Equilibrium Approximation to obtain the rate law. *e. Use the Steady-Sate Approximation to obtain the rate law.
2. What is the unit of k for each of the following type of reaction? First order reaction a. b. Second order reaction Third order reaction c.
Which statement is NOT correct? A. Activation energy is the same in the forward and reverse direction. B. The activated complex will be the highest on the reaction energy diagram. C. If the forward reaction is endothermic, the reverse reaction will be exothermic. D. In an endothermic reaction, the activation energy is usually greater than the change in enthalpy. E. An activated complex has higher energy than any molecule contributing to it.