At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.095M 'S NH,OH (aq) - NH, (aq)+H,0 (aq) Suppose a vessel contains NH,OH at a concentration of 1.19M. Calculate how long it takes for the concentration of NH,OH to decrease to 9.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.095M 'S NH,OH (aq) - NH, (aq)+H,0 (aq) Suppose a vessel contains NH,OH at a concentration of 1.19M. Calculate how long it takes for the concentration of NH,OH to decrease to 9.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
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Transcribed Image Text:O KINETICS AND EQUILIBRIUM
Brandon v
Using first- and second-order integrated rate laws
At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.095M
'S
NH,ОH (ад) -
NH, (ag) +н,о (аq)
Suppose a vessel contains NHOH at a concentration of 1.19M. Calculate how long it takes for the concentration of NH,OH to decrease to 9.0% of its initial
value. You may assume no other reaction is important.
dlo
Round your answer to 2 significant digits.
II
Expert Solution
Step 1
Given: Order of the reaction = 2.
Rate constant of the reaction = 0.095 M-1s-1.
Initial concentration of reactant NH4OH (i.e. A) = 1.19 M
And the final concentration of A = 9.0 % of initial concentration = 1.19 X 0.09 = 0.1071 M.
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