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Chemistry, 10.04.2020 04:59 angelinaviera09
The decomposition of nitramide, O 2 NNH 2 , O2NNH2, in water has the chemical equation and rate law O 2 NNH 2 ( aq ) โถ N 2 O ( g ) + H 2 O ( l ) rate = k [ O 2 NNH 2 ] [ H + ] O2NNH2(aq)โถN2O(g)+H2O(l)rate=k[O2NN H2][H+] A proposed mechanism for this reaction is O 2 NNH 2 ( aq ) k 1 โ k โ 1 O 2 NNH โ ( aq ) + H + ( aq ) ( fast equilibrium ) O2NNH2(aq)โkโ1k1O2NNHโ(aq)+H+(aq)(f ast equilibrium) O 2 NNH โ ( aq ) k 2 โโ N 2 O ( g ) + OH โ ( aq ) ( slow ) O2NNHโ(aq)โk2N2O(g)+OHโ(aq)(slow) H + ( aq ) + OH โ ( aq ) k 3 โโ H 2 O ( l ) ( fast ) H+(aq)+OHโ(aq)โk3H2O(l)(fast) What is the relationship between the observed value of k k and the rate constants for the individual steps of the mechaanism?
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The decomposition of nitramide, O 2 NNH 2 , O2NNH2, in water has the chemical equation and rate law...
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