Please show each step of each part carefully. Mechanism: Experiment shows that t
ID: 950666 • Letter: P
Question
Please show each step of each part carefully.
Mechanism: Experiment shows that the rate of formation of carbon tetrachloride from chloroform, CHCI_3+Cl_2(g) Rightarrow CCl_4(g)+HCl(g),is first order in CHCl_3 and 1/2 order in Cl_2 Determine which is the slow step from the following elementary steps. Show your work (i.e. solve for the rate law using the slow step). All steps are shown with equilibrium back and forth arrows, though one is the slow step. Step 1: Cl_2(g) 2Cl(g) Step 2: CI(g)+CHCl_3(g) HCI(g)+CCl_3(g) Step 3: CCl_3(g)+Cl(g) CCl_4(g) a) Write the experimental rate law (I.e. in the form of rate = k[A]^n[B]^m for this reaction. b) Write the rate law for each elementary step. Identify the intermediates. Write the backwards rate law if necessary. c) Using the information in parts a and b, identify the rate determining (slow) step for this reaction. Justify your choice by solving for the rate law of the slow step with no intermediates.Explanation / Answer
The followingmechanismhasbeenproposed forthe gas!phase reactionof chloroformCHCl3 and chlorine:
Cl2 (g) --------->2 Cl(g) (fast) , ( K1/K-1)
Cl(g) + CHCl3 (g)----------> HCl(g) + CCl3 (g) (slow) ,(K2)
Cl(g) + CCl3 (g) ------->CCl4 (g) (fast) , (K3)
Generally ,the step with rate slow rate is called rate determinating step.
a) the experimental rate law is , Rate = k2 [Cl][CHCl3]
b) Elementary reactions : the reactions in which are complete in 1 step are called elementary reactions.
rate law = K1[Cl2]
rate law = K-1[Cl] 2
rate law = Rate = k2 [Cl][CHCl3]
Rate = k3 [Cl][CCl3]
c)
Generally ,the step with slow rate is called rate determinating step.
the experimental rate law is , Rate = k2 [Cl][CHCl3]
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