Nitric oxide reacts with H_2 according to the | vedclass

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Question

(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: $Rate = -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d

Vedclass · Accepted Answer

$-\frac{1}{2} \frac{d[NO]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt} = \frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[H_2 O]}{dt}$

Vedclass · Answer

(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: $Rate = -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$.Applying this to the given reaction $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2 O_{(g)}$,we get:$Rate = -\frac{1}{2} \frac{d[NO]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt} = \frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[H_2 O]}{dt}$.Comparing this with the given options,option $A$ represents the correct stoichiometric relationship.

Nitric oxide reacts with $H_2$ according to the reaction: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2 O_{(g)}$. Identify the correct relation for the rate of disappearance of reactants and the rate of appearance of products.

Similar Questions

The term $\left( -\frac{dc}{dt} \right)$ in a rate equation refers to the:

For the following reaction in aqueous solution,what happens to the rate of reaction if $HCl$ is added?
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$

Assertion : Ionic reactions are not instantaneous.
Reason : Oppositely charged ions exert strong forces.

For a reaction $\frac{1}{2} A \rightarrow 2 B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by the expression:

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