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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solutionNH4+ + NO2→ N2 + 2 H2OExperiment0.7760.7761.551.55NO2l, M4.80x10-29.60x10-24.80×10-29.60x10-2Initial Rate, Ms11.29×10-52.58x10-52.57x10-55.15x10-4Complete the rate law for this reaction in the box below.Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01InRate =From these data, the rate constant is1--1

Question
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution
NH4+ + NO2
→ N2 + 2 H2O
Experiment
0.776
0.776
1.55
1.55
NO2l, M
4.80x10-2
9.60x10-2
4.80×10-2
9.60x10-2
Initial Rate, Ms1
1.29×10-5
2.58x10-5
2.57x10-5
5.15x10-4
Complete the rate law for this reaction in the box below.
Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01
In
Rate =
From these data, the rate constant is
1--1
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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2 → N2 + 2 H2O Experiment 0.776 0.776 1.55 1.55 NO2l, M 4.80x10-2 9.60x10-2 4.80×10-2 9.60x10-2 Initial Rate, Ms1 1.29×10-5 2.58x10-5 2.57x10-5 5.15x10-4 Complete the rate law for this reaction in the box below. Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01 In Rate = From these data, the rate constant is 1--1

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Determination of rate law for the given reaction

Given the reaction data

From experiment 1 and 2, [NH4+] is kept constant, [NO2-] is doubled, the rate also doubles

So, order with respect to [NO2-] = 1

From experiment 1 and 3, [NO2-] is constant, [NH4+] is doubled,...

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