Question

Which of the following statements is true for the reaction, ${H_2} + B{r_2} \to 2HBr$ . The rate law is $\dfrac{{dx}}{{dt}} = k[{H_2}]{[B{r_2}]^{\dfrac{1}{2}}}$ :
A.Order of reaction is 1.5
B.Molecularity of the reaction is 2.
C.By increasing the concentration of $B{r_2}$ four times the rate of reaction is doubled.
D.All of the above is correct.

Answer 1

The rate law for a chemical reaction is associated with an equation that links the initial or forward reaction rate with the concentration or pressure of reactants and constant parameters. Molecularity is additionally established on the rate of law. Molecularity of reaction is the number of molecules acting in the rate determining step while order of reaction.

Complete step by step answer:
The reaction occurs between hydrogen and bromine. Molecularity of reaction ${H_2} + B{r_2} \to 2HBr$ is 2, because here reactants have two molecules which are involved in the given elementary reactions.
Order of reaction realized by the rate of concentration. The order of reaction is that the relations between concentration and chemical reaction. Once the whole entire composition of the mixture within the species in the reaction is understood.
Here given the primary statement in keeping with the order of reaction. The order of reaction is:
=1+.05
=1.5
Molecularity of the reaction is 2 because it contains 2 moles of reactants.

Hence The correct answer is option (D).

Note:
The rate of law is derived by the equation of: $\dfrac{{dx}}{{dt}} = k[{H_2}]{[B{r_2}]^{\dfrac{1}{2}}}$ . It indicates that the concentration of $B{r_2}$ is increased and the rate of reaction is doubled. With rate of reaction, we know about the order of reaction and molecularity.