For the reaction $A_{(g)} + 3B_{(g)} \to 2C_{(g)}$,if the value of $-d[A]/dt$ is $3 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$,then the value of $-d[B]/dt$ will be:

Fill in the blanks:
$(a)$ The rate of reaction ....... as the concentration of reactant decreases.
$(b)$ The rate of reaction ....... as the concentration of product increases.

For the reaction: $A + 2 B \rightarrow C + D$,the expression for the rate of reaction is:

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)

Which of the following statements is correct?

In the reaction,$N_{2} + 3H_{2} \longrightarrow 2NH_{3}$,the rate of disappearance of $H_{2}$ is $0.02 \ M/s$. The rate of appearance of $NH_{3}$ is (in $M/s$)