A mass of #2.40*g# of calcium oxide is obtained by heating a mass of #5.00*g# calcium carbonate. What is the stoichiometric equation that represents the formation of calcium oxide, and what is the percentage yield?

Answer 1

We need a stoichiometrically balanced equation to represent the decomposition of calcium carbonate..........

#CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr#
The #Delta# symbol represents heat, and you have to fiercely heat these carbonates to effect decomposition. Note that this reaction is certainly stoichiometrically balanced: garbage in equals garbage out.
#"Moles of calcium carbonate "=" "(5.00*g)/(100.09*g*mol^-1)#
#=# #0.0500*mol#
#"Moles of calcium oxide "=" "(2.40*g)/(56.08*g*mol^-1)#
#=# #0.0428*mol#
#"% yield"# #=# #(0.0428*mol)/(0.0500*mol)xx100%=86%#

Are you content with this?

Keep in mind that most carbonates react to heat in this manner:

#MCO_3(s) + Delta rarr MO(s) + CO_2(g)uarr#
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Answer 2

The stoichiometric equation for the formation of calcium oxide from calcium carbonate is:

CaCO₃(s) → CaO(s) + CO₂(g)

The molar mass of CaCO₃ is 100.09 g/mol, and the molar mass of CaO is 56.08 g/mol.

The theoretical yield of calcium oxide can be calculated using stoichiometry:

1 mol of CaCO₃ produces 1 mol of CaO

Therefore, the theoretical yield of CaO is:

(5.00 g CaCO₃) / (100.09 g/mol CaCO₃) * (56.08 g/mol CaO) = 2.80 g CaO (theoretical yield)

The actual yield is given as 2.40 g.

Percentage yield = (actual yield / theoretical yield) * 100

Percentage yield = (2.40 g / 2.80 g) * 100 = 85.71%

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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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