Question

# The reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2- --->   N2...

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

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