$100 \, g$ $CaCO_3$ reacts with $1 \, L$ $1 \, N$ $HCl$. On completion of reaction,how much weight of $CO_2$ will be obtained? (in $g$)

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 $AgNO_3 = 170 \ g/mol$)

For the given reaction:
$CaCO_{3} + 2HCl \to CaCl_{2} + H_{2}O + CO_{2}$
If $90 \ g$ of $CaCO_{3}$ is added to $300 \ mL$ of $HCl$ solution which contains $38.55\%$ $HCl$ by mass and has a density of $1.13 \ g \ mL^{-1}$, then which of the following options is correct?
[Given molar masses of $H$, $Cl$, $Ca$, and $O$ are $1$, $35.5$, $40$, and $16 \ g \ mol^{-1}$ respectively]

$NH_3$ 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 $\%$)?

Calculate the amount of carbon dioxide that could be produced when
$(i)$ $1$ mole of carbon is burnt in air.
$(ii)$ $1$ mole of carbon is burnt in $16 \ g$ of dioxygen.
$(iii)$ $2$ moles of carbon are burnt in $16 \ g$ of dioxygen.

Balance the following chemical equations:
$(i)$ $Cu_2S + O_2 \to Cu_2O + SO_2$
$(ii)$ $Ca_3(PO_4)_2 + H_2SO_4 \to Ca(H_2PO_4)_2 + CaSO_4$