NEET 2018 Question Paper Mock Test

Consider the change in oxidation state of Bromine corresponding to different emf values:${\text{BrO}}_4^{-}\stackrel{1.82\text{V}}{\to }{\text{BrO}}_3^{-}\stackrel{1.5\text{V}}{\to }\text{HBrO}\stackrel{1.595\text{V}}{\to }{\text{Br}}_2\stackrel{1.0652\text{V}}{\to }{\text{Br}}^{-}$ The species undergoing disproportionation is:

For the redox reaction:$a{\text{MnO}}_4^{-}+b{\text{C}}_2{\text{O}}_4^{2-}+c{\text{H}}^{+}\to d{\text{Mn}}^{2+}+e{\text{CO}}_2+f{\text{H}}_2\text{O}$ The correct coefficients of the reactants $(a,b,c)$ for the balanced equation are:

Which one of the following conditions will favour maximum formation of the product in the reaction:$A_2(g)+B_2(g)\rightleftharpoons X_2(g)\Delta H=-X\text{kJ}$?

When initial concentration of the reactant is doubled, the half-life period of a zero order reaction:

The bond dissociation energies of $X_2,Y_2$ and $XY$ are in the ratio of $1:0.5:1$. $\Delta H$ for the formation of $XY$ is $-200{\text{kJ mol}}^{-1}$. The bond dissociation energy of $X_2$ will be: