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# Please help:Determine the overall orders of the reactions to which the following rate laws apply.?

(a) Rate = k[NO2]2

(b) Rate = k

(c) Rate = k[H2][Br2]1/2

(d) Rate = k[NO]2[O2]

answer choices to all problems:

a-zero order

b-first order

c-second order

d-third order

e-fourth order

f-0.5 order

g-1.5 order

### 1 Answer

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- 3 years agoFavorite Answer
Determining the overall order is done simply by adding up the exponents of the concentrations.

(a) Second order

**It only has [NO2] squared, so it's second

(b) Zero order

**This rate law has no concentration component, so there are zero exponents

(c) 1.5 order

**The exponent of [H2] is 1 and the exponent of [Br2] is 0.5. So added together, it is 1.5

(d) Third order

**The exponent of [NO] is 2 and the exponent of [O2] is 1. So added together, it is 3.

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