If the rate of reaction is given as $\frac{1}{3} \frac{d[X]}{dt} = -\frac{1}{2} \frac{d[Y]}{dt} = -\frac{d[Z]}{dt}$,the reaction can be represented as

Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$

For the reaction ${N_2}_{(g)} + 3{H_2}_{(g)} \to 2N{H_3}_{(g)}$,what is the relationship between $\frac{d[N{H_3}]}{dt}$ and $-\frac{d[{H_2}]}{dt}$?

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.

For a given chemical reaction $\gamma_{1} A + \gamma_{2} B \rightarrow \gamma_{3} C + \gamma_{4} D$,the rate of appearance of $D$ is $1.5$ times the rate of disappearance of $B$,which is twice the rate of disappearance of $A$. The rate of appearance of $D$ has been experimentally determined to be $9 \, mmol \, dm^{-3} s^{-1}$. Therefore,the rate of reaction is $...... \, mmol \, dm^{-3} s^{-1}$. (Nearest Integer)

The rate of a reaction that does not involve gases is not dependent on: