Which choice below is the rate law of the following reaction?
$2 H_{2} (g) + O_{2} (g) \to H_{2} O (g)$

R a t e = k [H] [O]

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R a t e = k [H_{2}]^{x} [O_{2}]^{y}

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R a t e = k [H_{2}]^{2} [O_{2}]

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R a t e = k [H_{2}] [O_{2}]

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Solution

The correct option is B $R a t e = k [H_{2}]^{x} [O_{2}]^{y}$
${2 H}_{2} (g) + O_{2} (g) ⟶ H_{2} O (g)$
The above reaction involves many intermediate species the rate law is determined form the slow-step process in a complex reaction. Therefore, We can predict the order of reaction. The order is determined experimentally.

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Similar questions

The chemical reaction $2 O_{3} \to 3 O_{2}$ involves two elementary steps :
$O_{3} f a s t - - \to O_{2} + O; O + O_{3} S l o w - -- \to 2 O_{2}$
The differential rate law expression will be :

Q. In the following reaction

2 H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}

rate of formation of

O_{2}

is 36g/min, what is the rate of disappearance

H_{2} O_{2}

Q. Find the order of reaction having rate law, rate =

k [N O]^{2} [H_{2}]

Q. The rate law for the reaction;

2 H_{2 (g)} + 2 N O_{(g)} \to N_{2 (g)} + 2 H_{2} O_{(g)}

\frac{d [N_{2}]}{d t} = k [H_{2}] [N O]^{2}

. Which of the following mechanisms is consistent with the rate law?

Q. Which of the following statement is true for the reaction,

H_{2} + {B r}_{2} \to 2 H B r

. The rate law is

\frac{d x}{d t} = k [H_{2}] {[{B r}_{2}]}^{1 / 2}

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Which choice below is the rate law of the following reaction?2H2(g)+O2(g)→H2O(g)

The correct option is B Rate=k[H2]x[O2]y2H2(g)+O2(g)⟶H2O(g)The above reaction involves many intermediate species the rate law is determined form the slow-step process in a complex reaction. Therefore, We can predict the order of reaction. The order is determined experimentally.

Which choice below is the rate law of the following reaction?
$2 H_{2} (g) + O_{2} (g) \to H_{2} O (g)$