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"#?

1 Answer
Aug 18, 2017

Answer:

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=??#