Determine the order and write the rate equation of the reaction between ammonium

Question

Determine the order and write the rate equation of the reaction between ammonium ion and nitrate ion in aqueous solution at 30 degrees C based on the following information about the rates of this reaction. (see photo)

The concentration of NH4+ is kept constant so that the initial rates of the reaction depend only on the concentration of the nitrite ion.

Problems 1. Determine in aqueous Brown, 1968) ine the order and write the rate equation tion between ammonium ion and nitrite ion us solution at 30°C based on the following tion about the initial rates of this reaction Concentration of NO2 mol/L 2.4 × 10-3 4.9 × 10-3 10.0 × 10-3 24.9 × 10-3 50.7 × 10-3 94.0 × 10-3 Initial rate mol L sec 18 x 10-s 33 x 10 65 × 10 156 × 10 338 x 10 NHJ + NO2 N2 + 2H2O The concentration of NH4 is kept constant so that the initial rates of the reaction depend only on the con entration of the nitrite ion. 643 x

Explanation / Answer

The given reaction is: NH4+ + NO2- N2 + 2H2O

Given that the concentration of NH4+ is kept constant and the initial rates of the reaction depend only on the concentration of nitrite ion.

Concentrations and respective initial rates are given in table. From the table we find that, on doubling the concentration of NO2- ion initial rate doubles.

Concentration of NO2- ion = 2.4x10-3 mol/L ; and initial rate = 18x10-8 mol/L s

On doubling the concentration we have:

Concentration of NO2- ion = 4.8x10-3 mol/L ; and initial rate = 36x10-8 mol/L s

Approximately the given values are matching so the order of the reaction is one.

That is n = 1.

The rate equation: -d[NO2-]/dt = k[NO2-]1

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