For the reaction $N_2 + 3H_2 \rightarrow 2NH_3$,if $\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,then what is the value of $-\frac{d[H_2]}{dt}$?

Consider the following reaction: $2 NO_{2(g)} + F_{2(g)} \longrightarrow 2 NO_2F_{(g)}$. The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are:

The reaction that occurs in a breath analyser,a device used to determine the alcohol level in a person's blood stream is $2 K_{2}Cr_{2}O_{7} + 8 H_{2}SO_{4} + 3 C_{2}H_{6}O$ $\rightarrow 2 Cr_{2}(SO_{4})_{3} + 3 C_{2}H_{4}O_{2} + 2 K_{2}SO_{4} + 11 H_{2}O$. If the rate of appearance of $Cr_{2}(SO_{4})_{3}$ is $2.67 \ mol \ min^{-1}$ at a particular time,the rate of disappearance of $C_{2}H_{6}O$ at the same time is ...... $mol \ min^{-1}$ (Nearest integer).

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:

In the reaction of formation of sulphur trioxide by contact process $2SO_2 + O_2 \rightleftharpoons 2SO_3$,the rate of reaction was measured as $\frac{d[O_2]}{dt} = -2.5 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of reaction in terms of $[SO_2]$ in $mol \ L^{-1} \ s^{-1}$ will be:

For the decomposition reaction $N_2O_{4(g)} \rightarrow 2NO_{2(g)}$,the initial pressure of $N_2O_4$ decreases from $0.46 \ atm$ to $0.28 \ atm$ in $30 \ minutes$. What is the rate of formation of $NO_2$?