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a) The reaction order in NO is 2

b) The reaction order in O₂ is 2

c) The overall order of the reaction is 4

d) If NO's concentration is halved, the reaction rate is quartered and is equal to 1.5 × 10⁴ M/s.

e) Reaction rate constant, k = 15.197 s/M³ = 15 s/M³ to 2s.f

Explanation:

The reaction order of a reaction with respect to a reactant is the power the reactant carries in the rate law.

a) The reaction order in NO is 2.

b) The reaction order in O₂ is 2.

c) Overall order is the sum of all the powers in the rate law, and for this reaction, it is 2 + 2 = 4

d) If the other parameters are constant, the rate of the reaction is directly proportional to the square of the concentration of NO

r = K [NO]²

At point 1, let r = r₁ and [NO] = [(NO)₁]

At point 2, let r = r₂ and [NO] = [(NO)₂]

r₁ = K [(NO)₁]²

At point 2,

r₂ = K [(NO)₂]²

But [(NO)₂] = [(NO)₁/2]

So, r₂ = K [(NO)₁/2]² = K [(NO)₁]²/4

And r₁ = K [(NO)₁]²,

So, r₂ = r₁/4

Meaning the reaction rate becomes (6.0 × 10⁴)/4 = 1.5 × 10⁴ M/s

e) The rate of the reaction is measured to be 79.0 M / s when [NO] = 1.2 M and [O2] = 1.9 M. Calculate the value of the rate constant.

r = k [NO]² [O₂]²

79 = k × 1.2² × 1.9²

k = 15.197 s/M³