By “the overall order of a reaction”,we mean

Which one of the following statements for the order of a reaction is incorrect?

$Zn + 2H^{+} \to Zn^{2+} + H_2$
The half-life period is independent of the concentration of zinc at constant $pH$. For the constant concentration of $Zn$,the rate becomes $100$ times when $pH$ is decreased from $3$ to $2$. Identify the correct statements $(pH = -\log [H^{+}])$:
$(A)$ $\frac{dx}{dt} = k[Zn]^0[H^{+}]^2$
$(B)$ $\frac{dx}{dt} = k[Zn][H^{+}]^2$
$(C)$ Rate is not affected if the concentration of zinc is made four times and that of $H^{+}$ ion is halved.
$(D)$ Rate becomes four times if the concentration of $H^{+}$ ion is doubled at constant $Zn$ concentration.

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

For a particular reaction,the rate expression is given as $r = k[A][B]^{0.5}$. If the volume of the vessel is reduced to one-fourth of the initial volume,the rate of reaction would

The rate law for the reaction $A + B \rightarrow C$ at $25^{\circ} C$ is given by $\text{rate} = k[A][B]^2$. Calculate the rate of reaction if the rate constant at the same temperature is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$ where $[A] = 1 \ M$ and $[B] = 0.2 \ M$.