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 ............... $mL$.

The amount of $BaSO_4$ formed upon mixing $100 \ mL$ of $20.8 \%$ $BaCl_2$ solution with $50 \ mL$ of $9.8 \%$ $H_2SO_4$ solution will be ............. $g$
( $Ba = 137, Cl = 35.5, S = 32, H = 1$ and $O = 16$ )

Moles of conc. $HNO_3$ required to oxidise one mole of sulphur is :
$S + 6HNO_3 \rightarrow H_2SO_4 + 6NO_2 + 2H_2O$

$5 \, \text{moles}$ of $A$,$6 \, \text{moles}$ of $B$,and an excess amount of $C$ are mixed to produce a final product $D$,according to the reactions:
$A + 2B \to I$
$I + C \to B + D$
What is the maximum number of moles of $D$ that can be produced,assuming that the products formed can be reused in the reactions?

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 $AgNO_3 = 169 \text{ g/mol}$, $KCl = 74.5 \text{ g/mol}$, $AgCl = 143.3 \text{ g/mol}$)

Combustion of $50 \ mL$ methane is carried out with $150 \ mL$ of air containing $21 \%$ oxygen by volume. What will be the total volume of the gaseous mixture after the reaction? (Assume water is in the gaseous state and air contains $79 \%$ nitrogen by volume).
$CH_{4(g)} + 2O_{2(g)} \to CO_{2(g)} + 2H_2O_{(g)}$