$5.8 \mathrm{g}$ of $\mathrm{NaCl}$ and $25.2 \mathrm{g}$ of ${\mathrm{AgNO}}_3$ are mixed together in aqueous solution form. What is the mass of silver chloride  $\left(\mathrm{AgCl}\right)$ ppt. formed according to the equation: 

${\mathrm{AgNO}}_3 \left(\mathrm{aq}\right)+\mathrm{NaCl}\left(\mathrm{aq}\right) \stackrel{}{\to } \mathrm{AgCl} \left(\mathrm{s}\right)+{\mathrm{NaNO}}_3\left(\mathrm{aq}\right)$

$(\mathrm{Ag}=108, \mathrm{N}=14, \mathrm{O}=16, \mathrm{Na}=23, \mathrm{Cl}=35.5)$

The equation for the burning of octane is:

$2{\mathrm{C}}_8{\mathrm{H}}_{18}+25{\mathrm{O}}_2 \stackrel{}{\to } 16{\mathrm{CO}}_2+18{\mathrm{H}}_2\mathrm{O}$

How many moles of carbon dioxide are produced when one mole of octane burns?

The equation for the burning of octane is:

What volume, at S.T.P; is occupied by $8$ moles of $C{O}_2.$

The equation for the burning of octane is:

If the relative molecular mass of carbon dioxide is $44$, what is the mass of carbon dioxide produced by burning two moles of octane?

The equation for the burning of octane is:

What is the empirical formula of octane?

The reaction given below takes place only in the gaseous state.

$4{\mathrm{N}}_2\mathrm{O}+{\mathrm{CH}}_4 \stackrel{}{\to } {\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}+4{\mathrm{N}}_2$

If all the volumes are measured at the same temperature and pressure, calculate the volume of dinitrogen oxide required to give $150 {\mathrm{cm}}^3$ of steam.

$2{\mathrm{C}}_4{\mathrm{H}}_{10}+13{\mathrm{O}}_2 \stackrel{}{\to } 8{\mathrm{CO}}_2+10{\mathrm{H}}_2\mathrm{O}$. Calculate:

How many moles of oxygen would be needed for the complete combustion of $5.8 \mathrm{g}$ of butane?

$2{\mathrm{C}}_4{\mathrm{H}}_{10} +13{\mathrm{O}}_2 \stackrel{}{\to } 8{\mathrm{CO}}_2+10{\mathrm{H}}_2\mathrm{O}.$Calculate:

What volume of ${\mathrm{CO}}_2$ at S.T.P is formed by complete combustion of $5.8 \mathrm{g}$ of butane?