# Question Which of the following is the correct rate law for this reaction? What will be the rate constant, k, for this reaction with proper units? Show all work. The following data was found for the reaction A+B Products Exp. Initial (A) Initial [B] Initial Rate M/S 1 0.015 0.022 0.125 2 0.030 0.044 0.500 3 0.060 0.044 0.500 4. 0.060 0.066 1.125 5 0.085 0.088 ?

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Transcribed Image Text: Which of the following is the correct rate law for this reaction? What will be the rate constant, k, for this reaction with proper units? Show all work. The following data was found for the reaction A+B Products Exp. Initial (A) Initial [B] Initial Rate M/S 1 0.015 0.022 0.125 2 0.030 0.044 0.500 3 0.060 0.044 0.500 4. 0.060 0.066 1.125 5 0.085 0.088 ?
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Transcribed Image Text: Which of the following is the correct rate law for this reaction? What will be the rate constant, k, for this reaction with proper units? Show all work. The following data was found for the reaction A+B Products Exp. Initial (A) Initial [B] Initial Rate M/S 1 0.015 0.022 0.125 2 0.030 0.044 0.500 3 0.060 0.044 0.500 4. 0.060 0.066 1.125 5 0.085 0.088 ?
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BPSUI7

Given reaction and data:A+Brarr Products According to rate law, rate equation can be written as:" Rate "=k[A]^(m)[B]^(n)Where, k is rate constant, R is rate and [A],[B] are respective concentration of reactants.Using given data (table), substitute respective values of [A], [B] and Initial rate (in above rate equation (X)) we get following rate equations; Now use different sets of any 2 equations from above table. (Note: for easier calculations use those 2 equations which contains same value concentration of either [A] or [B])Divide equation 3 by 4 ;{:[(0.500)/(1.125)=(k[0.060]^(m)[0.044]^(n))/(k[0.060]^(m)[0.066]^(n))],[0.444=([0.044]^(n))/([0.066]^(n))],[0.444=(0.667)^(n)],[0.444=(0.667)^(n)]:}Take log and solve for value of n :{:[log(0.444)=log{( ... See the full answer