Decay of $_{92}{U^{235}}$is .....order reaction

For a chemical reaction $A \to B$ it is found that the rate of reaction doubles, when the concentration of $A$ is increased four times. The order in $A$  for this reaction is

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

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$

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

Which of the following is correct