For the following reaction: OH^- + CH_3Br rightarrow CH_3OH + Br^- Imagine it is

Question

For the following reaction: OH^- + CH_3Br rightarrow CH_3OH + Br^- Imagine it is occurring in a solution where there are 1000 collisions every second between OH^- ions and CH_3Br molecules. Suppose only 7% of these collisions are sufficiently energetic to lead to products. Also assume that the orientation factor is 0.1. What is the rate of this reaction? Give your answer in the number of CH_3OH molecules formed per second. Write your answer in the box provided. You must show your work in order to receive credit. CH_3OH molecules formed/s

Explanation / Answer

rate of reaction = collision factor * energy factor * numbe rof collision
= 0.1* 7 % * 1000
= 0.1* 0.07 * 1000
= 7

Answer: 7

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