Consider the reaction A + B \rightarrow C and the following initial rates: Trial Initial Rate ...


Consider the reaction {eq}A + B \rightarrow C {/eq} and the following initial rates:

Trial Initial Rate {eq}(M sec^{-1}) {/eq} Initial Concentration of A (M) Initial Concentration of B (M)

1 {eq}3.8 \times 10^{-3} {/eq} 0.100 0.100

2 {eq}3.8 \times 10^{-3} {/eq} 0.100 0.150

3 {eq}5.7 \times 10^{-3} {/eq} 0.150 0.250

a) Calculate the order of the reaction with respect to A and B.

b) Calculate the rate constant.

c) Calculate the initial rate if a reaction is started with (A) = 0.2M and (B) = 0.8 M.

Rate Law and Order of Reaction

Rate Law suggests that the rate of a reaction is directly proportional to the concentration of reactants raised to the power which determines the order of the reaction. The overall order of a reaction is equal to the sum of orders with respect to each reactant.

{eq}P\ +\ Q\ \rightarrow\ M\\ Reaction\ Rate\ =\ k \left [ P \right ]^{m} \left [ Q \right ]^{n} {/eq}

where m and n are the order of reaction with respect to P and Q respectively.

Overall Order = m + n

Answer and Explanation: 1

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{eq}A\ +\ B\ \rightarrow\ C {/eq}

a) Order of reaction

Rate Law Equation :

{eq}Rate\ =\ k\left [A \right ]^{x} \left [B \right ]^{y} {/eq}


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Determining Rate Equation, Rate Law Constant & Reaction Order from Experimental Data


Chapter 35 / Lesson 2

Is your head spinning from rate laws, reaction orders and experimental data? Don't worry, this lesson will help you become a pro at all of these things by walking through two comprehensive problems that address all of these topics.

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