The order of a reaction which has the rate expression $\frac{{dc}}{{dt}} = K{[E]^{3/2}}{[D]^{3/2}}$ is

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

For a chemical reaction $A + B \rightarrow$ Product, the order is $1$ with respect to $A$ and $B$.

What is the value of $x$ and $y ?$

 $A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$  but it is independent of the concentration of $B$, then

The mechanism of the reaction $A + 2B \to D$ is

$2B\xrightarrow{k}{B_2}$        [Slow]

${B_2} + A \to D$          [Fast]

The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order are respectively

For the reaction $A \to B$, the rate law expression is : Rate $ = \,k\,[A]$ Which of the following statements is incorrect