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(B) The gas described is $N_2$ (nitrogen). $1$. It is almost inert at room temperature due to the very high bond dissociation energy of the $N \equiv

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nitrogen

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(B) The gas described is $N_2$ (nitrogen). $1$. It is almost inert at room temperature due to the very high bond dissociation energy of the $N \equiv N$ triple bond $(941.4 \ kJ \ mol^{-1})$. $2$. It is used to create an inert atmosphere in electric bulbs to prevent the oxidation of the tungsten filament. $3$. The combustion of nitrogen to form nitrogen oxides is an endothermic process (e.g.,$N_2(g) + O_2(g) \rightarrow 2NO(g)$,$\Delta H > 0$),which is unusual as most combustion reactions are exothermic.

$A$ gas at low temperature does not react with most compounds. It is almost inert and is used to create an inert atmosphere in bulbs. The combustion of this gas is exceptionally an endothermic reaction. Based on the given information,we can conclude that the gas is

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