If a sample of $8.3 \ mL$ of $H_2SO_4$ $(36 \ N)$ is diluted with $991.7 \ mL$ of water,what is the approximate concentration of the resulting solution (in $N$)?

Calculate the approximate mass (in $g$) of $H_2S$ required for the following reaction when $15 \ L$ of oxygen at $STP$ reacts completely.
$2 H_2S_{(g)} + 3 O_{2(g)} \longrightarrow 2 SO_{2(g)} + 2 H_2O_{(g)}$
(molar mass of $H_2S = 34 \ g \ mol^{-1}$)

What will be the normality of a solution containing $4.9 \ g$ of $H_3PO_4$ dissolved in $500 \ mL$ water (in $N$)?

If $50 \ mL$ of $0.5 \ M$ oxalic acid is required to neutralize $25 \ mL$ of $NaOH$ solution, the amount of $NaOH$ in $50 \ mL$ of the given $NaOH$ solution is . . . . . . $g$.

The formula of a gaseous hydrocarbon which requires $6$ times of its own volume of $O_{2}$ for complete oxidation and produces $4$ times its own volume of $CO_{2}$ is $C_{x}H_{y}$. The value of $y$ is $......$ .

$A$ mixture of $H_2$ and $O_2$ at $1 \, atm$ pressure contains $20 \%$ by weight of $H_2$. Find out the partial pressure of $H_2$ in $atm$.