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If the rate law for a reaction is rate = k[A]2[B]
a. What is the overall order of the reaction?
b. If the concentration of A is doubled and the concentration of B is tripled, how will this affect the rate of the reaction?
c. How will doubling the concentration of B while holding A constant affect the value of k (assuming that temperature remains constant)?
under identical conditions 2-bromopropane reacts with iodide ionin acetone at a rate that is 105 faster than the rate
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