The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism

$(i)$ $X + Y \rightleftharpoons M$      very rapid equilibrium

$(ii)$ $M + Z \to P$      slow

$(iii)$ $O + Y \to N$      very fast

What is the rate law for this reaction

The reaction, ${N_2}{O_5} \longrightarrow 2NO + \frac{1}{2}\,{O_2}$ is of first order for $N_2O_5$ with rate constant $6.2 \times 10^{-4}\, s^{-1}$. what is the value of rate of reaction when $[N_2O_5] = 1.25\, mol\, L^{-1}$

For a chemical reaction $Y + 2Z \to $ Product, rate controlling step is $Y\, + \frac{1}{2}Z\, \to Q$  If the concentration of $Z$ is doubled, the rate of reaction will

Write general reaction. Write rate law of general reaction.

For the reaction $3\,{A_{\,(g)\,}}\,\xrightarrow{K}\,{B_{(g)}}\, + \,\,{C_{(g)\,,}}K$ is ${10^{ - 14}}\,L/mol.\min .$ if $(A) = 0.5\,M$ then the value of $ - \frac{{d(A)}}{{dt}}$ (in $M / sec$ ) is.

For the reaction $2NO_2 + F_2 \to 2NO_2F$ , following mechanism has been provided

$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$

$N{O_2} + F\xrightarrow{{fast}}N{O_2}F$

Thus rate expression of the above reaction can be written as