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Helen [10]
2 years ago
8

The rate law for 2NO(g) + O₂(g) → 2NO₂(g) is rate = is rate k[NO]²[O₂]. is rateIn addition to the mechanism in the text (p. 709)

, the following ones have been proposed:2NO(g) + O₂(g) → 2NO₂(g)2NO(g) ⇄ N₂O₂(g) [fast]N₂O₂(g) + O₂(g) → 2NO₂(g) [slow]2NO(g) ⇄ N₂(g) + O₂(g) [fast]N₂(g) + 2O₂(g) → [slow](b) Which of these mechanisms is most reasonable? Why?
Chemistry
1 answer:
KonstantinChe [14]2 years ago
5 0

The rate law depicts the effect of concentration on reaction rate. Second mechanism 2NO(g) ⇄ N₂O₂(g) [fast], N₂O₂(g) + O₂(g) → 2NO₂(g) [slow] is most reasonable. Thus, option b is correct.

<h3>What is rate law?</h3>

Rate law and equation give the rate at which the reaction takes place under the influence of the concentration of the reactants. The balanced chemical reaction is given as,

2NO(g) + O₂(g) → 2NO₂(g)

The rate of the equation is given as,

rate = k [NO]² [O₂]  

In a multi-step chemical reaction, the slowest step is the rate-determining step. The second mechanism is given as,

2NO (g) → N₂O₂ (g) [fast]

N₂O₂(g) +O₂(g) → 2NO₂ (g) [slow]

Rate is given as,

rate = k [N₂O₂] [O₂]

Therefore, option b. the second mechanism is the most reasonable.

Learn more about rate law, here:

brainly.com/question/14779101

#SPJ4

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