For the chemical reaction $N_{2(g)} + 3 H_{2(g)} \rightleftharpoons 2 NH_{3(g)}$,the correct option is
- A$-\frac{1}{3} \frac{d[H_{2}]}{dt} = -\frac{1}{2} \frac{d[NH_{3}]}{dt}$
- B$-\frac{d[N_{2}]}{dt} = 2 \frac{d[NH_{3}]}{dt}$
- C$-\frac{d[N_{2}]}{dt} = \frac{1}{2} \frac{d[NH_{3}]}{dt}$
- D$3 \frac{d[H_{2}]}{dt} = 2 \frac{d[NH_{3}]}{dt}$
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Similar Questions
For the following reaction in aqueous solution,what happens to the rate of reaction if $HCl$ is added?
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$
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Mention the factors that affect the rate of a chemical reaction.
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