The reaction:
${CH}_{3} COF + H_{2} O \to {CH}_{3} COOH + HF$

has been studied under the following initial conditions.

$CASE I : CASE II : C_{H_{2} O} = 1.00 M C_{H_{2} O} = 0.02 M . C_{{CH}_{3} COF} = 0.01 M C_{{CH}_{3} COF} = 0.80 M$
Concentrations were monitored as a function of time and are given below:

Determine the order of the reaction and the rate constant for the reaction.

Solution

Let rate k(C_CH₃COF)^a(C_H₂O)^bC_H₂O >> C_CH₃COFand in the second case, C_H₂O << C_CH₃COF. In the first case we determine the order of the reaction with respect to CH₃ COF. We note that the reaction is not of zero order as rate of reaction changes with time.

Therefore k(C_H₂O) = 0.0154 min^–1 and we note the order of reaction with respect to CH₃COF is 1.
Now we determine the order of raction with respect to water.
Again,

The reaction is first order in H₂O and we have

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Chemical Kinetics

Some More Questions From Chemical Kinetics Chapter

The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?

What will be the effect of temperature on rate constant?

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