Please show all work and formulas - Thank You The following elementary steps are

Question

Please show all work and formulas - Thank You

The following elementary steps are determined to be the mechanism of a given reaction Step 1 (slow): A B C+D Step 2 (fast): CE Step 3 (fast) E A3B+F a. What is the overall reaction? O A+BC+D 2A + B + 2C + E- + C + D + E + F b. Which species is are intermediate(s)? (If more than one species are intermediates, enter them separated by a single space.) c. What is the rate law for step 1 of this mechanism? (Do not use spaces in your answer. For zero order, don't include the reactant for first order, don't include the order.) rate d. What is the rate law for step 3 of this mechanism? (Do not use spaces in your answer. For zero order, don't include the reactant; for first order, don't include the order.) rate e. What is the molecularity of step 1? f. What is the rate law for the overall reaction? (Do not use spaces in your answer. For zero order, don't include the reactant for first order, don't include the order) rate-

Explanation / Answer

a)

overall reaction can be obtained by adding all steps.

A + B + C + E + A —> C + D + E + 3B + F

After removing common compound:

A + B + A —> D + 3B + F

2 A —> D + 2B + F

Answer: option 1

b)

C is intermediate since it is produced in step 1 and used up in step 2

E is intermediate since it is produced in step 2 and used up in step 3

Answer: C E

c)

rate law for step 1 is:

rate = k[A][B]

d)

rate law for step 3 is:

rate = k[E][A]

e)

in step 1, there are two reactant each with coefficient 1

So, molecularity = 2

f)

rate depends on the slowest step

Here 1st step is slowest

So, rate law is same as rate law of step 1

Hence rate law is:

rate = k[A][B]

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