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Be sure to answer all parts. Determine the overall orders of the reactions to which the following rate laws apply: (a) rate = k[NO2]2 (b) rate = k zero order first order 1.5 order second order 2.5 order third order zero order first order 1.5 order second order 2.5 order third order (c) rate = k[H2][Br2]1/2 (d) rate = k[NO2]2[O2] zero order first order 1.5 order second order 2.5 order third order zero order first order 1.5 order second order 2.5 order third order

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sebassandin

Answer:

(a). second order.

(b). zeroth order.

(c). one and a half order.

(d). third order.

Explanation:

Hello,

In this case, you just have to add the concentration's powers in each rate law:

(a) [tex]r=k[NO_2]^2[/tex]

Just the 2-power is present, so it is a second order law.

(b) [tex]r=k[/tex]

No power is present, so it is a zeroth order law.

(c) [tex]r=k[H_2]*[Br_2]^{1/2}[/tex]

1 plus 1/2 gives 1.5, that is why it is a 1.5 (one and a half) order law.

(d) [tex]r=k[NO_2]^2[O_2][/tex]

2 plus 1 gives 3, that is why it is a third order law.

Best regards.

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