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hichkok12 [17]
3 years ago
11

A sample of 53.0 of carbon dioxide was obtained by heating 1.31 g of calcium carbont. What is the percent yield for this reactio

n?
CaCO3 ? CaO + CO2
Chemistry
1 answer:
MaRussiya [10]3 years ago
6 0

Answer:

92.04%

Explanation:

Given:

Mass of CO₂ obtained = 53.0 grams

Mass of calcium carbonate heated = 1.31 grams

Now,

the molar mass of the calcium carbonate = 100.08 grams

The number of moles heated in the problem = Mass  / Molar mass

= (1.31 grams) / (100.08 grams/moles)

= 0.013088 moles

now,

1 mol of calcium carbonate yields 1 mol of CO₂

thus,

0.013088 moles of calcium carbonate will yield = 0.013088 mol of CO₂

now,

Theoretical mass of 0.013088 moles of CO₂ will be

= Number of moles × Molar mass of CO₂

= 0.013088 × 44 = 0.5758  grams

Thus, the percent yield for this reaction = \frac{\textup{Actual yield}}{\textup{Theoretical yield}}\times100

or

the percent yield for this reaction = \frac{0.53}{0.5758}\times100

or

the percent yield for this reaction = 92.04%

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3 years ago
Calculate the number of moles of caco3 (calcium carbonate, or limestone) in a 20.0g sample of this substance
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First calculate for the molar mass of the given formula unit, CaCO₃. This can be done by adding up the product when the number of atom is multiplied to its individual molar mass as shown below.

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