Among $CaH_2, BeH_2 , BaH_2,$ the order of ionic character is

Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below :

Then the species undergoing disproportionation is

For the redox reaction
$MnO_4^-+C_2O_4^{2-}+H^+\rightarrow Mn^{2+} +CO_2 + H_2O$
The correct coefficients of the reactants for the balanced equation are
$MnO_4^-$ $C_2O_4^{2-}$ $H^+$

Which one of the following conditions will favour maximum formation of the product in the reaction,
$A_2(g)+B_2(g)\rightleftharpoons X_2(g)\triangle_r H=-XKJ?$

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. ΔH for the formation of XY is –200 kJ $mol^{–1}$. The bond dissociation energy of $X_2$ will be

The correction factor ‘a’ to the ideal gas equation corresponds to

Consider the following species :
$CN^+, CN^–, NO$ and CN
Which one of these will have the highest bond order?

Magnesium reacts with an element (X) to form an ionic compound. If the ground state electronic configuration of (X) is $1s^2 2s^2 2p^3$, the simplest formula for this compound is

Iron exhibits bcc structure at room temperature. Above 900°C, it transforms to fcc structure. The ratio of density of iron at room temperature to that at 900°C (assuming molar mass and atomic radii of iron remains constant with temperature) is