In a reaction $A_2B_{3(g)} \to A_{2(g)} + \frac{3}{2}B_{2(g)}$,the pressure increases from $60 \ torr$ to $75 \ torr$ in $2.5 \ min$. The rate of disappearance of $A_2B_3$ is ........ $torr \cdot min^{-1}$.

For the reaction $\frac{1}{2} A \rightarrow 2B$,the rate of disappearance of $A$ is related to the rate of appearance of $B$ by which of the following expressions?

For the reaction $2A + B \rightarrow 3C + D$,which of the following does not express the rate of reaction?

In a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$

The rate of a chemical reaction can be expressed in terms of:

For a chemical reaction $4 A + 3 B \rightarrow 6 C + 9 D$,the rate of formation of $C$ is $6 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$ and the rate of disappearance of $A$ is $4 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. The rate of reaction and the amount of $B$ consumed in an interval of $10 \ s$,respectively,will be: