In the reaction $2A + B \to {A_2}B$, if the concentration of $A$ is doubled and of $B$ is halved, then the rate of the reaction will

Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$

Which is True $(T)$ and False $(F)$ in the following sentence ?

The order of this reaction is $1$.

For a reaction $2A + B \to $ Products, doubling the initial concentration of both the reactants increases the rate by a factor of $8$, and doubling the concentration of $+B$  alone doubles the rate. The rate law for the reaction is

For a given reaction ${t_{1/2}} = \frac{1}{{Ka}}.$. The order of the reaction is

The value of $\frac{{{t_{0.875}}}}{{{t_{0.50}}}}$ for $n^{th}$ order reaction 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 $=k\left[ CH _{3} CHO \right]^{3 / 2}$