Reaction 1: A first order reaction (A à products) has the rate constant k = 0.483 min-1 (Rate = k[A]), and the initial concentration of reactant A is 0.800 M. Reaction 2: A second order reaction (B à products) has the rate constant k = 0.483 M-1 min-1 (Rate = k[B]2), and the initial concentration of reactant B is 0.800 M. Which of the following statements is true about these two reactions? Choose one option only Options: a. Reaction 1 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 2 will.
Here we compare the first order and second order reaction based on Integrative rate laws.
Reaction 1: A first order reaction (A à products) has the rate constant k = 0.483 min-1 (Rate = k[A]), and the initial concentration of reactant A is 0.800 M.
Reaction 2: A second order reaction (B à products) has the rate constant k = 0.483 M-1 min-1 (Rate = k[B]2), and the initial concentration of reactant B is 0.800 M.
Which of the following statements is true about these two reactions?
Choose one option only
Options:
a. Reaction 1 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 2 will.
b. Reaction 2 will take less time to change the reactant concentration from 0.800 M to 0.400 M than Reaction 1 will.
c. Reaction 1 and Reaction 2 will take the same amount of time to change the reactant concentration from 0.800 M to 0.400 M.
d. None of the above
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