the following data were obtained: 5.25x103 441 2.63x103 661 NHa], M 1.05x102 1.3
ID: 572020 • Letter: T
Question
the following data were obtained: 5.25x103 441 2.63x103 661 NHa], M 1.05x102 1.32x103 seconds Hint: It is not necessary to graph these data. The observed half life for this reaction when the starting concentration is 1.05x10 Mis 441 concentration is 5.25x10 Mis 221 s and when the starting The average rate of disappearance of NH3 from t = 0 s to t = 441 s is | 1.19x10^-5 Ms The average rate of disappearance of NH3 from t = 441 s to t = 661 s is | 1.19x10^-5 M s Based on these data, the rate constant for this zero order reaction is | 1.19x10^-5 An error has been detected in your answer. Check for typos miscalculations etc. before submitting your answer Submit Answer Retry Entire Group 6 more group attempts remaining Previous NextExplanation / Answer
1) Half life when the starting concentration is 1.05 x 10-2 M.
Half life is the time taken when the concentration becomes half of the initial.
Half concentration = (1.05 x 10-2)/2 M = 5.25 x 10-3M
From the table the time taken from the initial conc 1.05 x 10-2 M to become half 5.25 x 10-3M is
= 441- 0 seconds = 441 seconds
Similarly, if the starting concentration is 5.25 x 10-3M. then time taken to becoming the concentration half i.e.
=(5.25 x 10-3)/2 = 2.63 x 10-3M will be
= 661 - 441 = 220 seconds
2)Average rate of dissapearance of NH3 from t=0 sec to t=441 seconds:
= [1.05 x 10-2 - 5.25 x 10-3]/ 441
= 1.19 x 10-5 Ms-1.
3)Average rate of dissapearance of NH3 from t=441 sec to t=661 seconds:
= [5.25 x 10-3 - 2.63 x 10-3]/ 220
= 1.19 x 10-5 Ms-1.
4) Yes the order of reaction is zero order and for zero order half life
t1/2= [A]0/ 2k
441s = 1.05 x 10-2M/ 2k
k = 1.19 x 10-5 Ms-1.
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