In the given reaction, ; $K_3 > K_2 > K_1$

then rate determining step will be

For a reaction, $AB_5 \to AB + 4B$ The rate can be expressed in following ways

$\frac{{ - d[A{B_5}]}}{{dt}} = K[A{B_5}]$ ;    $\frac{{d[B]}}{{dt}} = {K_1}[A{B_5}]$

So the correct relation between $K$ and $K_1$ is

For a certain reaction, the rate $=k[A]^2[B]$, when the initial concentration of $A$ is tripled keeping concentration of $B$ constant, the initial rate would

The specific rate constant of a first order reaction depends on the

The alkaline hydrolysis of ethyl acetate is represented by the equation$C{H_3}COO{C_2}{H_5} + NaOH \to C{H_3}COONa + {C_2}{H_5}OH$ Experimentally it is found that for this reaction$\frac{{dx}}{{dt}} = k[C{H_3}COO{C_2}{H_5}]\,[NaOH]$ Then the reaction is

In a reaction involving hydrolysis of an organic chloride in presence of large excess of water$RCl + {H_2}O \to ROH + HCl$