Under similar conditions of pressure and temperature,$40 \, mL$ of slightly moist hydrogen chloride gas is mixed with $20 \, mL$ of ammonia gas,the final volume of gas at the same temperature and pressure will be ............. $mL$.

$50.0 \, kg$ of $N_2 \, (g)$ and $10.0 \, kg$ of $H_2 \, (g)$ are mixed to produce $NH_3 \, (g)$. Calculate the amount of $NH_3 \, (g)$ formed. Identify the limiting reagent in the production of $NH_3$ in this situation.

The mass of $AgCl$ precipitated when a solution containing $11.70 \ g$ of $NaCl$ is added to a solution containing $3.4 \ g$ of $AgNO_3$ is [Atomic mass of $Ag=108$,$Na=23$,$Cl=35.5$,$N=14$,$O=16$] (in $g$)

Calculate the number of moles of oxygen required to react with $6.8 \, g$ of ammonia in the following reaction:
$NH_3 + O_2 \to NO + H_2O$

$NH_3$ is produced according to the following reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$. In an experiment,$0.25 \ mol$ of $NH_3$ is formed when $0.5 \ mol$ of $N_2$ is reacted with $0.5 \ mol$ of $H_2$. What is the percentage yield (in $\%$)?

$3O_2 + 2N_2 \to 2N_2O_3$
$9 \ mol$ of $O_2$ and $14 \ mol$ of $N_2$ are allowed to react. When $3 \ mol$ of $O_2$ remains unreacted,how many moles of $N_2O_3$ would have been produced?