$A$ car airbag is inflated by $N_2$ produced during rapid decomposition of $NaN_{3(s)}$. What will be the pressure of the inflated airbag if $130 \ g$ of $NaN_3$ is used (in $atm$)? The volume of the airbag is $10 \ L$ $(T = 300 \ K, R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$.

Concentrated aqueous sulfuric acid is $98\%$ $H_2SO_4$ by weight and has a density of $1.80 \ g \ mL^{-1}$. The volume of acid required to make $1 \ L$ of $0.1 \ M$ $H_2SO_4$ solution is ....... $mL$.

$5 \, N$ $H_2SO_4$ was diluted from $1 \, L$ to $10 \, L$. The normality of the solution obtained is.....$N$.

$20 \ mL$ of $0.2 \ M \ Al_2(SO_4)_3$ is mixed with $20 \ mL$ of $6.6 \ M \ BaCl_2$. The concentration of $Cl^{-}$ ion in the final solution is $......... \ M$.

When $5 \ L$ of a gas mixture of methane and propane is perfectly combusted at $0 \ ^\circ C$ and $1 \ atm$,$16 \ L$ of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in $kJ$ ($\Delta H_{comb.} (CH_4) = 890 \ kJ \ mol^{-1},$ $\Delta H_{comb.} (C_3H_8) = 2220 \ kJ \ mol^{-1}$) is

What is the volume occupied by $2.5 \ mol$ of ammonia gas at $\text{STP}$ (in $dm^3$)?