Consider the following reaction: A+B→C+D The initial concentrations of the reactants A and B are 0.220 M and 0.320 M, respectively. The rate of reaction is 0.060 M⋅S-1, and the orders of the reaction, with respect to reactants A and B, are 1 and 2, respectively. Determine the rate constant (k) for the reaction using the rate law. Express your answer in M-2⋅S-1 to three significant figures.
Answer:-
This question is solved by using the simple concept of chemical kinetics which involves the determination of rate of reaction.
The answer is given in the image,
Consider the following reaction: A+B→C+D The initial concentrations of the reactants A and B are 0.220...
3C/a0596e8ecf339a3.. sion < > 5 of 19 Review | Constants | Periodic Table Consider the following reaction: A+BC+D The initial concentrations of the reactants A and B are 0.380 M and 0.260 M, respectively. The rate of reaction is 0.060 M S, and the orders of the reaction, with respect to reactants A and B, are 1 and 2, respectively. Determine the rate constant (k) for the reaction using the rate law. 2 Express your answer in M figures. to...
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