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7 October, 09:54

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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  1. 7 October, 12:06
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    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
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