(a) Calculate the order of reaction. CHEMICAL KINETICS 101 (b) Write rate law. (c) Calculate the rate constant of the reaction. [Ans. 1, \( 3 \times 10^{-2} \mathrm{~min}^{-1} \) ]
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- The order of reaction is given as 1. This means the reaction is first-order with respect to the reactant. Show more…
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(a) Given these data for the reaction $\mathrm{A}+\mathrm{B} \longrightarrow \mathrm{C}$, write the rate-law expression. (b) What is the value, with units, for the specific rate constant? $$ \begin{array}{cccc} & \begin{array}{c} \text { Initial [A] } \\ (M) \end{array} & \begin{array}{c} \text { Initial [B] } \\ (M) \end{array} & \begin{array}{c} \text { Initial Rate of } \\ \text { Formation of C } \\ (M / \mathrm{s}) \end{array} \\ \hline 1 & 0.10 & 0.10 & 2.0 \times 10^{-4} \\ 2 & 0.10 & 0.20 & 8.0 \times 10^{-4} \\ 3 & 0.20 & 0.40 & 2.56 \times 10^{-2} \end{array} $$
For the reaction $\mathrm{A} \longrightarrow$ products The following data are obtained. (a) Determine the order of the reaction. (b) Write the rate expression for the reaction. (c) Calculate $k$ for the experiment above.
A chemical reaction is expressed by the balanced chemical equation: A + 2B -> C Consider the data: Initial [A] (M) Initial [B] (M) Initial rate (M/min) 0.21 0.21 0.00290795 0.21 0.42 0.0116318 0.42 0.42 0.0232636 A. Find the rate law for the reaction. B. Calculate the value of the specific rate constant. C. If the initial concentrations of both A and B are 0.41 M, at what initial rate is C formed?
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