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oksian1 [2.3K]
3 years ago
9

Consider the following reaction: CHCl3(g) + Cl2(g) → CCl4(g) + HCl(g) The initial rate of the reaction is measured at several di

fferent concentrations of the reactants with the following results: [CHCl3] (M) [Cl2] (M) Initial rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, choose the correct rate law for the reaction. rate=k[CHCl3][Cl2]2 rate=k[CHCl3][Cl2]12 rate=k[CHCl3]2[Cl2] rate=k[CHCl3]12[Cl2]
Chemistry
1 answer:
Ira Lisetskai [31]3 years ago
7 0

Answer : The correct rate law for the reaction is,

\text{Rate}=k[CHCl_3][Cl_2]^{1/2}

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

For the given chemical equation:

CHCl_3(g)+Cl_2(g)\rightarrow CCl_2(g)+HCl(g)

Rate law expression for the reaction:

\text{Rate}=k[CHCl_3]^a[Cl_2]^b

where,

a = order with respect to CHCl_3

b = order with respect to Cl_2

Expression for rate law for first observation:

0.0035=k(0.010)^a(0.010)^b ....(1)

Expression for rate law for second observation:

0.0069=k(0.020)^a(0.010)^b ....(2)

Expression for rate law for third observation:

0.0098=k(0.020)^a(0.020)^b ....(3)

Expression for rate law for fourth observation:

0.027=k(0.040)^a(0.040)^b ....(4)

Dividing 1 from 2, we get:

\frac{0.0069}{0.0035}=\frac{k(0.020)^a(0.010)^b}{k(0.010)^a(0.010)^b}\\\\2=2^a\\a=1

Dividing 2 from 3, we get:

\frac{0.0098}{0.0069}=\frac{k(0.020)^a(0.020)^b}{k(0.020)^a(0.010)^b}\\\\1.42=2^b\\b=\frac{1}{2}

Calculation used :

1.42=2^b\\\log (1.42)=b\log 2\\\log (\frac{1.42}{2})=b\\b=0.5=\frac{1}{2}

Thus, the rate law becomes:

\text{Rate}=k[CHCl_3]^1[Cl_2]^{1/2}

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