Nitrous acid (HNO2) slowly decomposes to NO, NO2, and water by the following second-order reaction: 2 HNO2(aq) ---> NO(g) + NO2(g) + H2O(l) Use the date below to determine the rate law and the constant for this reaction: Time (s) [HNO2] (um) 0 0.1560 1000 0.1466 1500 0.1424 2000 0.1383 2500 0.1345 3000 0.1309 A) Rate = ?? B) k = ??? /uM*s C) Determine the half-life for the decomposition of HNO2: t1/2 = ?

The rate law of the reaction will be given as;

The value of rate constant of the reaction is :

The half life for the decomposition of is 15,596.73 s

Explanation:

Given that reaction follows second order kinetics;

The rate law of the reaction will be given as;

Integrated rate law for second order kinetics is given by:

= initial concentration

A = concentration left after time t

k = rate constant of the reaction

Concentration at 0 second:

Concentration at 1000 second:

t = 1000 s - 0 s = 1000 s

Half life for second order kinetics is given by:

So, the half life for the decomposition of :

The half life for the decomposition of is 15,596.73 s

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