5

Question 53ptsFor the reaction shown below, if Cl- is produced at a rate of 3.6 Ms 1,at what rate is CIO consumed?3 CIO (aq) _+2 Cl (aq) CIOa (aq)4.7Ms1.9 Ms 15.4 M...

Question

Question 53ptsFor the reaction shown below, if Cl- is produced at a rate of 3.6 Ms 1,at what rate is CIO consumed?3 CIO (aq) _+2 Cl (aq) CIOa (aq)4.7Ms1.9 Ms 15.4 Ms-16.2Ms

Question 5 3pts For the reaction shown below, if Cl- is produced at a rate of 3.6 Ms 1,at what rate is CIO consumed? 3 CIO (aq) _+2 Cl (aq) CIOa (aq) 4.7Ms 1.9 Ms 1 5.4 Ms-1 6.2Ms



Answers

Consider the reaction, $$\mathrm{CH}_{3} \mathrm{Cl}(g)+3 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g)+3 \mathrm{HCl}(g)$$ (a) Express the rate of the reaction with respect to each of the reactants and products. (b) If the instantaneous rate of the reaction with respect to $\mathrm{HCl}$ is $0.029 \mathrm{M} \mathrm{s}^{-1}$, what is the instantaneous rate of the reaction?

Mm. So another do a problem like this. You have to look at the story commentary after reaction and we know that he's telling the story documentary. Okay. Okay. Based on this documentary Uh rate of disappearance of roaming when divided by five. 10 to O. B. R minus. Yeah it went into T. So negative of this. It was reacted is equal to one divided by three. Then we are to grooming which is the product. So we are given that this part. Okay, here's 3.500 in this part of -4. So this is equal to one divided by three concentration of roaming. The tight straight of formation of roaming. If you want to play. By the way this was negative and negative so they're going to cancel to become positive and therefore mhm. Three Divided by five, multiplied by 3.5 entertained this power of -4 which is 2.1 entertain this power of -4 more belligerent per second.

Well, everyone, this is Ricky. And today we're working on a problem number six from chapter 12. So we're giving this reaction and using the Easter geometry and our knowledge that the rate of disappearance for br minuses 3.5 times 10 to the negative forth more per second, we have to calculate the right of formation of e. R. Two. And so the easiest way to think about this is that, um, the rate of formation of B R two is so for every five b r minus, we get three b r two. So using this ratio, we can calculate the rate of formation sometimes. So this is right of disappearance of B R, minus times three b R. Two over five B minus hoop waas. And now just running through the calculation, you see that the rape of formation is 2.1 times 10 to the negative third born per second. So this video is helpful

Hey, I said in this question were given the reaction where A and B are forming C and D, and we're given that a is second order and B is your order were also given the re constant for this reaction. And we want to know what the rate of reaction is when we're given a concentration of A and B. So to do this all first right out my rate law, my general rate law. So that is my rate is going to be equal to my constant times the concentration of a to some order times concentration of B to some order. Now, we are already given all the values we need to solve this. So I'm gonna go ahead and plug those in. So we're giving our K, which is 0.103 in verse Moeller inverse minutes as its units were also given that a has a concentration of 0.116 Mohler and that's to the second power. And since B is to the zero power, anything to the zero power is one. We don't have to worry about its concentration. So now that we have that, I can go ahead and plug this into my calculator. And the rate of this reaction with these given concentrations is 1.39 times 10 to the negative fourth moller per minute, and this is my final answer.

For this question, we have a generic reaction of a plus B goes to C plus D. They tell us that it is second order in a and zero order in B that then give us the rate constant to be 0.103 one over Moller minutes. It then asks, What is the rate of this reaction when we have a given a concentration and a given be concentration? To answer this question, we're going to use the differential rate law or just the rate law itself. The rate is equal to K multiplied by a raised to its order which is second to multiplied by be raised to its order, which is zero because it's zero order. Anything raised to the zero is one. So it essentially cancels from our rate law. So right then will be equal to K, which is provided at 0.0 mhm one throw three and then multiplied by the concentration which is provided at 0.116 Moller and we're going to square that this will give us a rate of 1.39 times 10 to the negative four Mueller per minute


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