If $0.5 \ mol$ of $BaCl_2$ is mixed with $0.1 \ mol$ of $Na_3PO_4$,what is the maximum number of moles of $Ba_3(PO_4)_2$ formed?

What is the approximate mass of the precipitate formed when $50 \text{ mL}$ of $16.9\%$ solution of $AgNO_3$ is mixed with $50 \text{ mL}$ of $7.45\%$ $KCl$ solution (in $\text{ g}$)? (Molar mass of $AgNO_3 = 169 \text{ g/mol}$, $KCl = 74.5 \text{ g/mol}$, $AgCl = 143.3 \text{ g/mol}$)

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

When $22.4 \ L$ of $H_{2(g)}$ is mixed with $5.6 \ L$ of $Cl_{2(g)}$,each at $S.T.P.$,the moles of $HCl_{(g)}$ formed after completion of the reaction is closest to $.... \ mol$.

Assume carbon burns according to the following equation:
$2C_{(s)} + O_{2(g)} \rightarrow 2CO_{(g)}$
When $12 \ g$ of carbon is burnt in $48 \ g$ of oxygen,the volume of carbon monoxide produced is $...... \times 10^{-1} \ L$ at $STP$ [nearest integer].
[Given: Assume $CO$ as an ideal gas,molar mass of $C = 12 \ g \ mol^{-1}$,molar mass of $O = 16 \ g \ mol^{-1}$,and molar volume of an ideal gas at $STP$ = $22.7 \ L \ mol^{-1}$]

The heat of neutralisation of a strong acid and a strong base is $13.7 \ kcal$. The heat released when $0.6 \ mole$ $HCl$ solution is added to $0.25 \ mole$ of $NaOH$ is: (in $kcal$)