Upon heating, calcium carbonate decomposes to produce calcium oxide and carbon dioxide. What is the theoretical yield of #CO_2# if 235.0 g #CaCO_3# is heated?

Answer 1

Approx. 100 g of carbon dioxide gas are evolved.

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

The molar equivalence of carbonate to carbon dioxide is therefore 1:1.

#"Moles of calcium carbonate"# #=# #(235.0*g)/(100.0869*g*mol^-1)# #=# #2.35# #mol#.
So, by reaction stoichiometry, #2.35# #mol# #CO_2(g)# are evolved.
If conversion is quantitative, there are #2.35# #mol# #xx# #44.0*g*mol^-1# #CO_2# #=# #??g#
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Answer 2

The molar mass of CaCO₃ is 100.09 g/mol. The balanced equation is:

CaCO₃ → CaO + CO₂.

Calculate moles of CaCO₃: 235.0 g / 100.09 g/mol = 2.349 moles.

Theoretical yield of CO₂: 2.349 moles × 1 mol CO₂/1 mol CaCO₃ = 2.349 moles CO₂.

Convert moles to grams: 2.349 moles × 44.01 g/mol = 103.29 g CO₂.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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