The mass of ammonia in grams produced when $2.8 \ kg$ of dinitrogen quantitatively reacts with $1 \ kg$ of dihydrogen is.............

Complete combustion of ethane gives only gaseous products. In a closed vessel,$15 \ g$ of ethane and $112 \ g$ of $O_2$ were allowed to completely react. What is the total number of moles of gaseous substances present in the vessel at the end of the reaction?

Identify the values of $A$, $B$, $C$, $D$ and $E$ for the following unbalanced reaction: $aKNO_3 + 5C_{12}H_{22}O_{11} \rightarrow bN_2 + cCO_2 + dH_2O + eK_2CO_3$

An electric discharge is passed through a mixture containing $50 \ mL$ of $O_{2(g)}$ and $50 \ mL$ of $H_{2(g)}$. The volume of the product $(H_2O)$ formed at $110 \ ^oC$ will be ............... $mL$.

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation:
$N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$
$(i)$ Calculate the mass of ammonia produced if $2.00 \times 10^{3} \, g$ of dinitrogen reacts with $1.00 \times 10^{3} \, g$ of dihydrogen.
$(ii)$ Will any of the two reactants remain unreacted?
$(iii)$ If yes,which one and what would be its mass?

$0.4 \text{ g}$ of dihydrogen is made to react with $7.4 \text{ g}$ of dichlorine to form hydrogen chloride. The volume of hydrogen chloride formed at $273 \text{ K}$ and $1 \text{ bar}$ pressure is: (in $\text{ L}$)