The reaction of ammonium ion with nitrite ion in aqueous
solution
NH4+ + NO2- --->
N2 + 2
H2O
is first order in
NH4+ and
first order in
NO2-.
Complete the rate law for this reaction.
Use the form k[A]m[B]n... ,
where '1' is understood for m, n ... (don't enter
1) and concentrations taken to the zero power do not
appear.
Rate = |
In an experiment to determine the rate law, the rate of the
reaction was determined to be 1.64×10-5
Ms-1 when [NH4+]
= 0.914 M and
[NO2-] =
5.08×10-2 M. From this experiment, the
rate constant is M-1s-1.
NH4+ + NO2- ---> N2 + 2 H2O
first order in NH4+ and first order in NO2-.
Rate law
Rate = K[NH4^+]^1[NO2^-]^1
The rate of the reaction was determined to be 1.64×10-5 Ms-1
[NH4+] = 0.914 M and [NO2-] = 5.08×10-2 M.
Rate = K[NH4^+]^1[NO2^-]^1
1.64*10^-5 = K(0.914)^1(5.08*10^-2)^1
K = 1.64*10^-5/(0.914)(5.08*10^-2)
= 0.000353M^-1 s^-1
= 3.53*10^-4 M^-1 s^-1 >>>>answer
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