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BartSMP [9]
3 years ago
5

How is an endothermic reaction identified?

Chemistry
2 answers:
Fynjy0 [20]3 years ago
6 0
D- It requires heat as a reactant
AnnZ [28]3 years ago
3 0

Answer: It requires heat as a reactant.

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A possible mechanism for the overall reaction Br2 (g) + 2NO (g) → 2NOBr (g) is NO (g) + Br2 (g) rightwards arrow with k space 1
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Answer : The rate law for formation of NOBr based on this mechanism is, \frac{k_1\times k_2}{k_1^-}[Br_2][NO]^2

Explanation :

The overall reaction is:

Br_2(g)+2NO(g)\rightleftharpoons 2NOBr(g)

Rate law = k[Br_2][NO]^2

The first step of the overall reaction is:

NO(g)+Br_2(g)\overset{k_1}{\rightarrow} NOBr_2(g)

NO(g)+Br_2(g)\overset{k_1^-}{\leftarrow} NOBr_2(g)

Rate law 1 = k_1[Br_2][NO]

Rate law 2 = k_1^-[NOBr_2]

The second step of the overall reaction is:

NOBr_2(g)+NO(g)\overset{k_2}{\rightarrow} 2NOBr

Rate law 3 = k_2[NOBr_2][NO]

Now rate law of overall reaction can be obtained as follows.

We are multiplying rate law 1 and rate law 3 and dividing by rate law 2, we get:

Rate law = \frac{[k_1[Br_2][NO]]\times [k_2[NOBr_2][NO]]}{[k_1^-[NOBr_2]]}

Rate law = \frac{k_1\times k_2}{k_1^-}[Br_2][NO]^2

Rate law = k[Br_2][NO]^2

The rate law for formation of NOBr based on this mechanism is, \frac{k_1\times k_2}{k_1^-}[Br_2][NO]^2

4 0
3 years ago
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