Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO₃) into solid calcium oxide and gaseous carbon dioxide. Suppose 23.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 380.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Be sure your answer has the correct number of significant digits.

Question

Camden Barajas

Chemistry

12 November, 06:38

Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO₃) into solid calcium oxide and gaseous carbon dioxide. Suppose 23.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 380.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Be sure your answer has the correct number of significant digits.

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Harrison Ashley · Answer 1

CaCO3 (s) → CaO (s) + CO2 (g)

The mass of carbonate that must have reacted was 43.03 grams

Explanation:

CaCO3 → CaO + CO2

Relation between reactant and product is 1:1

Let's apply the Ideal Gas Law to find out the moles of CO2 which were produced.

P. V = n. R. T

1 atm. 23 L = n. 0.082 L. atm/mol. K. 653K

(1atm. 23L) / (0.082 mol. K/L. atm. 653K) = n

0.43 moles = n

0.43 moles of CO2, were produced from 0.43 moles of CaCO3.

Molar weight of CaCO3 = 100.08 g/m

Mass = Molar weight. moles

Mass = 100.08 g/m 0.43 m = 43.03 g