During a chem lab experiment we studied a bleach/dye reaction from a pseudo firs
ID: 880006 • Letter: D
Question
During a chem lab experiment we studied a bleach/dye reaction from a pseudo first-order kinetics standpoint. During the experiment we used one drop of brilliant-blue (BB) dye in bleach solution at different temperatures and recorded the time it took for each to decolorize. Can someone explain how this experiment can be modified to study the bleach/dye reaction at an overall second-order kinetics standpoint? During a chem lab experiment we studied a bleach/dye reaction from a pseudo first-order kinetics standpoint. During the experiment we used one drop of brilliant-blue (BB) dye in bleach solution at different temperatures and recorded the time it took for each to decolorize. Can someone explain how this experiment can be modified to study the bleach/dye reaction at an overall second-order kinetics standpoint?Explanation / Answer
Rate law - The rate of a reaction can be represented either by the disappearance of reactants or the appearance of products.
rate = -d[A]/ dt = k[A]^x
where x = 0,1,2,3 ......
Zero oder reaction - These are reactions whose rate does not change when the concentration of a reactant changes.
rate = k [A]^0
rate = K
second oder reaction-This is where the rate of a reaction is proportional to the concentration of one species by a factor of 2; or two species by a factor 1 so that 1+1 = 2
rate= k[A]^2 or k [A][B]
in this reaction of beach/dye when it is second oder the decolorization of beach solution is depends on the concentration of bleach solution and amount of dye used. We can record the time of decolorization of solution keeping concentration of one reactant constant that is two times concentration of bleach solution is kept constant & amoun of dye is changed. And two times amount of dyes is kept constant &concentration of bleach solution is changed time of decolourization is noted in each case.
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