(a) Which of the following is the correct rate law for the forward reaction in s
ID: 818601 • Letter: #
Question
(a) Which of the following is the correct rate law for the forward reaction in step (1)?
rate = k1[A]2
rate = k-1[A2]
rate = k1[A]2 - k-1[A2]
rate = k1 Ý 2 Ý [A]
(b) Which of the following is the correct rate law for the reverse reaction in step (1)?
rate = k-1[A]2
rate = k-1[A2]
rate = -k1[A2]
rate = -k-1[A]2
(c) Which of the following is the rate law for the rate-determining step?
rate = k2[A2][E]
rate = k2[A2][E]-k-1[A2]
rate = k1[A]2 + k-1[A2] + k2[A2][E]
none of the above
(d) Which of the following is the correct chemical equation for the net reaction that occurs in this chemical change?
2A + E --> B + C
2A + A2 + E --> B + C
2A + E + A --> A + B + C
None of the above
(e) Use the results of parts (a) and (b) to identify the rate law of the rate-determining step in terms of the concentrations of the reactants in the overall balanced equation for the reaction.
none of the answers are correct
in which the first step is a very rapid reversible reaction that can be considered to be essentially an equilibrium (forward and reverse reactions occurring at the same rate) and the second is a slow step.
Suppose a reaction occurs with the following mechanism: in which the first step is a very rapid reversible reaction that can be considered to be essentially an equilibrium (forward and reverse reactions occurring at the same rate) and the second is a slow step.
Explanation / Answer
rate = k1[A]2 - k-1[A2]
rate = k1[A]2 - k-1[A2]
rate = -k1[A2]
rate = k1[A]2 + k-1[A2] + k2[A2][E]
2A + E + A --> A + B + C
rate = k2 Ý (k-1/k1) Ý [A]2[E]
rate = k1[A]2 - k-1[A2]
rate = k1[A]2 - k-1[A2]
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