The following experimental data were obtained for the reaction of NH4+ and NO2¯ in acidic solution.NH4+ (aq) + NO2 (aq) → N2(g) +2 H2O(4)[NH, *] (mol L-) NO,¯] (mol L-) Rate = A[N2]/At (mol L-1s-1)0.00170.1305.53 x 10-80.00170.0652.76 x 10-80.00900.2605.86 x 10-70.00460.2602.98 x 10-7Determine the rate law for this reaction.(Use k for the rate constant.)Rate =Calculate the rate constant.Rate constant =

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Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =

Chemistry

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Chapter1: Chemical Foundations

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The following experimental data were obtained for the reaction of NH4+ and NO2¯ in acidic solution.
NH4+ (aq) + NO2 (aq) → N2(g) +2 H2O(4)
[NH, *] (mol L-) NO,¯] (mol L-) Rate = A[N2]/At (mol L-1s-1)
0.0017
0.130
5.53 x 10-8
0.0017
0.065
2.76 x 10-8
0.0090
0.260
5.86 x 10-7
0.0046
0.260
2.98 x 10-7
Determine the rate law for this reaction.
(Use k for the rate constant.)
Rate =
Calculate the rate constant.
Rate constant =

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[H2O2 (aq)], M 0.0850 0.170 0.250 0.350 0.350 0.350 0.350 [l* (aq)], M 0.100 0.100 0.100 0.100 0.200 0.300 0.400 A [H₂O₂ (aq)] At 1.4 2.9 4.2 5.9 12 18 24 -, (M-s¯¹) x 10-4
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