The following energy diagram is the reaction progress for the reaction: (CHg)3CCI + OH" → (CH3)3COH + cr at 45 °C. The energy diagram shows that the reaction mechanism has 2 steps. These 2 steps have the same orientation factors and same number of collisions per second. Which of the following statements concerning the mechanism is correct? 135 kJ- 115 kJ 90 kJ -25 kJ- (CH),CCI + OH reactants -60 kJ + (CH),COH + CF products reaction coordinate (progress of reaction) If a catalyst is added to the above reaction at 45 °C, the rate of the reaction will increase and the heat O a. (enthalpy) of the reaction will decrease for the forward reaction. b. In the mechanism of the above reaction, the activation energy of the first step is 135 k). O c.In the mechanism of the above reaction, the first step is most likely the rate determining step. d. The overall reaction of this reaction is endothermic. e. When the temperature is increased, the activation energy of both steps will decrease. Energy

The following energy diagram is the reaction progress for the reaction: (CHg)3CCI + OH" → (CH3)3COH + cr at 45 °C. The energy diagram shows that the reaction mechanism has 2 steps. These 2 steps have the same orientation factors and same number of collisions per second. Which of the following statements concerning the mechanism is correct? 135 kJ- 115 kJ 90 kJ -25 kJ- (CH),CCI + OH reactants -60 kJ + (CH),COH + CF products reaction coordinate (progress of reaction) If a catalyst is added to the above reaction at 45 °C, the rate of the reaction will increase and the heat O a. (enthalpy) of the reaction will decrease for the forward reaction. b. In the mechanism of the above reaction, the activation energy of the first step is 135 k). O c.In the mechanism of the above reaction, the first step is most likely the rate determining step. d. The overall reaction of this reaction is endothermic. e. When the temperature is increased, the activation energy of both steps will decrease. Energy

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.96PAE: The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g)...

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Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
(Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
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