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Chapter 13: Problem 155

Write the overall balanced chemical equation that goes along with the mechanism: Elementary step 1: \(\mathrm{Cl}_{2} \rightarrow 2 \mathrm{Cl}\) Elementary step \(2: \mathrm{Cl}+\mathrm{CHCl}_{3} \rightarrow \mathrm{HCl}+\mathrm{CCl}_{3}\) Elementary step \(3: \mathrm{Cl}+\mathrm{CCl}_{3} \rightarrow \mathrm{CCl}_{4}\)

Short Answer

Expert verified
The overall balanced chemical equation for the given mechanism is: \(\mathrm{Cl}_{2} + \mathrm{CHCl}_{3} \rightarrow \mathrm{HCl} + \mathrm{CCl}_{4}\).

Step by step solution

01

Write down the elementary steps

Begin by listing the elementary steps given in the problem: Elementary step 1: \(\mathrm{Cl}_{2} \rightarrow 2 \mathrm{Cl}\) Elementary step 2: \(\mathrm{Cl}+\mathrm{CHCl}_{3} \rightarrow \mathrm{HCl}+\mathrm{CCl}_{3}\) Elementary step 3: \(\mathrm{Cl}+\mathrm{CCl}_{3} \rightarrow \mathrm{CCl}_{4}\)
02

Add the elementary steps

Now we add the elementary steps to obtain the overall equation: \(\mathrm{Cl}_{2} + \mathrm{Cl}+\mathrm{CHCl}_{3} + \mathrm{Cl}+\mathrm{CCl}_{3} \rightarrow 2 \mathrm{Cl} + \mathrm{HCl}+\mathrm{CCl}_{3} + \mathrm{CCl}_{4}\)
03

Cancel out species present on both sides

We can observe that there are species on both sides that can be canceled out. They are: - 2 moles of \(\mathrm{Cl}\) atoms, appearing on both the left and right sides - 1 mole of \(\mathrm{CCl}_{3}\), appearing on both the left and right sides Since these species are present on both sides of the equation, they are considered intermediates and can be canceled out from the overall equation: \(\cancel{2 \mathrm{Cl}} + \cancel{\mathrm{CCl}_{3}}\) After canceling out the intermediates, we are left with: \(\mathrm{Cl}_{2} + \mathrm{CHCl}_{3} \rightarrow \mathrm{HCl} + \mathrm{CCl}_{4}\)
04

Final overall balanced chemical equation

Now that we have canceled out all the intermediates in the overall equation, we have the final overall balanced chemical equation: \(\mathrm{Cl}_{2} + \mathrm{CHCl}_{3} \rightarrow \mathrm{HCl} + \mathrm{CCl}_{4}\)

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Most popular questions from this chapter

Which of the following will slow down a chemical reaction? (a) Increase concentration of reactants. (b) Add catalyst. (c) Decrease temperature. (d) All of the above.

What do we mean by activation energy?

The rate of a reaction depends both on inherent factors and on concentration. The rate constant \(k\) is associated with the inherent factors. What are they?

\(\Delta E_{\mathrm{rxn}}\) for the reaction \(\mathrm{X} \rightarrow \mathrm{Y}\) is \(+30 \mathrm{~kJ}\). (a) Is the reaction endothermic or exothermic? (b) Rewrite the reaction showing heat as either a reactant or a product. (c) What is the value of \(\Delta E_{\mathrm{rxn}}\) for the reverse reaction \(\mathrm{Y} \rightarrow \mathrm{X} ?\) (d) Is the reverse reaction endothermic or exothermic? (e) Will the container in which the forward reaction \(\mathrm{X} \rightarrow\) Y occurs feel hot or cold to the touch? Why?

Would decreasing the size of \(E_{a}\) increase or decrease the rate of a reaction? Explain your choice fully.
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