$1.44 \ g$ of titanium (At. wt. $= 48$) reacted with excess of $O_2$ to produce $x \ g$ of a non-stoichiometric compound $Ti_{1.44}O$. The value of $x$ is:

In the reaction,$2Al_{(s)} + 6HCl_{(aq)} \rightarrow 2Al^{3+}_{(aq)} + 6Cl^{-}_{(aq)} + 3H_{2(g)}$

In the reaction $2 KClO_{3(s)} \longrightarrow 2 KCl_{(s)} + 3 O_{2(g)}$,$\Delta H^{\circ} = -78 \ kJ$. If $33.6 \ L$ of oxygen gas is liberated at $S.T.P.$,what is the mass of $KCl_{(s)}$ produced (in $g$)? (Atomic mass: $K = 39, Cl = 35.5 \ g \ mol^{-1}$)

What is the stoichiometric ratio of the products in the reaction: $3K_2MnO_4 + 2H_2SO_4 \rightarrow 2KMnO_4 + 2K_2SO_4 + MnO_2 + 2H_2O$?

How many $ml$ of $1 \, (M) \, H_2SO_4$ are required to neutralize $10 \, ml$ of $1 \, (M) \, NaOH$ solution?

What is the volume of $4.4 \ g$ of $CO_2$ at $STP$ in $L$?