Question

What volume of carbon dioxide would evolve from fierce heating of a `200*g` mass of `"calcium carbonate"` on heating under standard conditions of `"STP"`?

Answer 1

Well, `"STP"` specifies a temperature of `273.15*K` and an absolute pressure of exactly `100 *kPa`. I gets under `50*L`.

Explanation:

We interrogate the decomposition reaction....

`CaCO_3(s) + Delta rarrCaO(s) + CO_2(g)uarr`

And given complete decomposition we have a molar quantity of `(200*g)/(100.09*g*mol^-1)=2.0*mol` WITH RESPECT TO CALCIUM CARBONATE, AND CARBON DIOXIDE. And as you know this molar quantity also represents a (large!) number with respect to gaseous molecules.

And the volume expressed by this quantity is simply given by the old Ideal Gas equation..`V=(nRT)/P`

`-=(2.0*molxx0.0821*(L*atm)/(K*mol)xx273.15*K)/((100*kPa)/(101.3*kPa*atm^-1))`

`=??*L`

And the number of molecules is simply `2*molxx6.022xx10^23*mol^-1=??`