$56 \ g$ of $CaO$ has been mixed with $63 \ g$ of $HNO_3$. The amount of $Ca(NO_3)_2$ formed is: (in $g$)

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$
$(i)$ 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?

$KMnO_4$ reacts with $KI$ in basic medium to form $I_2$ and $MnO_2$. When $250 \ mL$ of $0.1 \ M \ KI$ solution is mixed with $250 \ mL$ of $0.02 \ M \ KMnO_4$ in basic medium, what is the number of moles of $I_2$ formed?

Calcium carbonate reacts with aqueous $HCl$ to give $CaCl_2$ and $CO_2$ according to the reaction given below: $CaCO_{3(s)} + 2HCl_{(aq)} \to CaCl_{2(aq)} + CO_{2(g)} + H_2O_{(l)}$
What mass of $CaCl_2$ will be formed when $250 \ mL$ of $0.76 \ M$ $HCl$ reacts with $1000 \ g$ of $CaCO_3$? Name the limiting reagent. Calculate the number of moles of $CaCl_2$ formed in the reaction.

What should be the weight and moles of $AgCl$ precipitate obtained on adding $500 \ mL$ of $0.20 \ M$ $HCl$ to $30 \ g$ of $AgNO_3$ solution (in $g$)? (Molar mass of $AgNO_3 = 170 \ g/mol$)

$A$ $10.0 \, L$ vessel contains $O_2$ at a partial pressure of $600 \, torr$ and $H_2$ at a partial pressure of $400 \, torr$. The gases react according to the following equation upon electric sparking: $H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(g)}$. If the reaction goes to completion,which of the following is correct?