20.0 g of calcium carbonate is heated to produce carbon dioxide according to the equation CaCO3(s) → CaO(s) + CO2(g)?

Question

20.0 g of calcium carbonate is heated to produce carbon dioxide according to
the equation
CaCO3(s) → CaO(s) + CO2(g)
If the reaction is carried out at a temperature of 800.0 degrees C and a constant pressure of
1.0 atm is maintained, what volume of carbon dioxide gas is recovered?

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Answer 1 · 2016-05-22T06:18:22

#CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr#

There are #(20.0*g)/(100.0*g*mol^-1)# #=# #0.20*mol*CaCO_3#

Given the stoichiometry, an equivalent molar quantity of carbon dioxide gas will be evolved.

At #1# #atm# pressure, and #1073*K#, this gas will have a volume of:

#V=(nRT)/P# #=# #(0.20*molxx0.0821*L*atm*K^-1*mol^-1xx1073*K)/(1*atm)#

#=# #??L#