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Experiment 2 Pre-Lab QuestionsIf the = concentration of Cl, is halved, then the reaction rate would factor ofConsider the following graphs of In k versus 5 for reac...

Question

Experiment 2 Pre-Lab QuestionsIf the = concentration of Cl, is halved, then the reaction rate would factor ofConsider the following graphs of In k versus 5 for reactions A, B,Cand D.Which reaction ofthe four (A,B,C,or D) would have the largest activation energy? Explain the rationale for your answer:

Experiment 2 Pre-Lab Questions If the = concentration of Cl, is halved, then the reaction rate would factor of Consider the following graphs of In k versus 5 for reactions A, B,Cand D. Which reaction ofthe four (A,B,C,or D) would have the largest activation energy? Explain the rationale for your answer:



Answers

Consider the two reactions:
a. Why is the activation barrier for the first reaction so much
higher than that for the second?
b. The frequency factors for these two reactions are very close
to each other in value. Assuming that they are the same,
calculate the ratio of the reaction rate constants for these two
reactions at 25 C.

This question wants you to consider the general reaction or generic reaction of E plus F. Goes to G plus H. With the following reaction coordinate diagram. When considering this, it wants you to identify which of the following statements are true, the first statement is the activation energy is greatest for the forward direction. This would be false. The activation energy in the reverse direction, which is the difference in energy between here and here is greater than it is in the forward direction. Which we the difference from here to here. So in the reverse direction, it's greater in the forward direction. The difference in energy from here to here is less and the activation energy is the energy required to go up the hill dependent upon the direction you're traveling. So the activation energy is greatest actually in the reverse direction. Next one is B. The reactant are at a lower energy than the products. That is also false. The reactant, which are these ones are at a higher energy than the products due to their position in the reaction coordinate next statement, see the reaction is end A thermic. This is also false If we end up going from a higher energy state to a lower energy state. When we go from reactant to products, energy must be released. This would correspond to an exotic thermic reaction, not an end a thermic reaction statement. D The rate of the forward reaction would be slowed by an increase in temperature. This is also false. The rate of the forward and reverse reactions are both increased with an increase in temperature. All rates are increased when we increased temperature not slowed when we increased temperature. If we talk about the position of equilibrium, that's another issue. But if we're just talking about the rate in the forward direction that will that will increase with an increase in temperature not decrease or be slowed And the last one is E. If the rate law for the reaction is rate is equal to K. Multiplied by E squared, multiplied by F, Then doubling the concentration of E will cause the rate to increase by a factor of four. So if this goes from one 22, then we're going from one squared, Which equals 1-2 squared which equals four. So that is correct that doubling the concentration of E will cause the rate to increase by a factor of four. This statement is true.

Here's a rough sketch of the energy diagram. Well, obviously referred to the book for more precise one, but this is the energy in killer jewels as the reaction makes progress. And we can see for part A. Because the products have higher energy than the reactant it's going to be. And a thermic some energy was absorbed in the course of the reaction. Then for part B. Um We want to know the energy for the forward reaction. So we'll compare the energy of the reactant and product looks like the reactions are about zero and the products are about at 25. Um So that's an increase of positive 25 killer dolls. For part C. We want to know the activation energy. So let's say that it's at about 65 at the top. As an approximation here, this would be about 65 what we're going with. So the activation energy in the forward direction is going to be from 0 to 65 um is going to be 65 killer jewels. And then in the reverse direction we would go from where the products are to the little peek. So from 25 to 65 that would be 40 kg jewels would be required in the reverse direction. Then for part D. If a catalyst lowers the activation energy. Um Bye. Uh 10 kg joules. It's going to lower the activation energy of both the forward and the rivers. So you can imagine that we draw another curve where it would be like around 55. So would be something like that. Um So the amount of energy needed to go from products to the peak would be lower. And then the rate of the forward reaction, I mean the reverse reaction yeah would increase. So we'll put rate of the reverse increases in the presence of a catalyst. Mhm.

In Probleble 37 of Chapter two. Chemical Kinetics and Equilibrium. Yeah. So we have Cuban in this question, A reaction in which A plus B. Can react for C. And the rate law Yeah. Can be written as R. Is equal to K. Concentration of a scare into concentration of K. No. According to question doubling the concentration of A without changing concentration of be increased the rate of reaction by. So if we double the concentration of a the concentration of me as it is. So I can write this four times K into concentration of a scare into concentration of P. So this assume as the the A dish. So red assumed the kurdish. So our dish is equal to. So this is equal to our. So it means we can see the rate of reaction Increased by four pinks. So I can write the reaction is of second order. Mhm. With respect to A. Yeah And doubling the concentration of a, increases the rate of reaction by four times. So I can't write doubling the concentration money. Mhm increases the rate of reaction by four times. Mhm. So option see Option B four times. Is that correct?

In problem 45 entrepreneur to chemical kinetics and equilibrium. So in this question we have given a rate law of our reaction which is R. Is equal to K. And to concentration of a scare into concentration of B. So now in the question it is said that doubling the concentration of both A and B increases the rate of reaction, so on doubling the concentration of A. And be. So if we double the concentration of N. B. Then the rate of reaction that is represented by R. Dash is equal to K. Into twice of concentration of a whole scare into price of concentration of B. So this can be written as K. Into four concentration of a whole scale into two into concentration of B. So this becomes eight into K. Into concentration of a scare into concentration of P. And we know this value that is equal to Uh huh. So our dash is equal to eight times are So hence we can see that the rate of reaction rate of reaction increased by eight times. So hence since the reaction is of second order, since reaction is second order with respect to a and first order with respect to the, so the rate of reaction increased by so the route of reaction increased by increased by eight times, so increased by eight times. So it means from the given option option number C. Is the correct. So we can write option C increases each times is the correct? Yeah.


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