For a reaction between substances $A$ and $B$,the rate law is given by: $\text{Rate} = K[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,what will be the ratio of the new rate to the original rate?

If the concentration of the reactants is increased,the rate of reaction

Reaction: $KClO_3 + 6FeSO_4 + 3H_2SO_4 \to KCl + 3Fe_2(SO_4)_3 + 3H_2O$
Which is True $(T)$ and False $(F)$ in the following statement?
The order of this reaction is $1$.

Consider the following reactions:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is:

In the sequence of reaction $A$ $\xrightarrow{k_1} X$ $\xrightarrow{k_2} Y$ $\xrightarrow{k_3} Z$ with $k_3 > k_2 > k_1$,then the rate determining step is

Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. Which of the following conditions does $NOT$ affect the rate of reaction?