Problemas
Calcium carbonate decomposes to form calcium oxide and carbon dioxide according to the reaction: CaCO_(3)(s)arrow CaO(s)+CO_(2)(g) . What mass of calcium oxide is produced from the decomposition of 23.6 g of calcium carbonate? (23.6gCaCO_(2))/(100.gCaOCl_(3))times (1molCaO)/(1molCaOO_(2))times (56.1gCaO)/(1molCaO)=132g Number 5 is a preview of the types of calculations you'll learn to do in this worldaudd
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Salvador
veterano · Tutor durante 12 años
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(282 Votos)
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The correct answer is 132 g of calcium oxide.Explanation:The balanced chemical equation for the decomposition of calcium carbonate (CaCO3) is:CaCO3(s) → CaO(s) + CO2(g)Given that 23.6 g of calcium carbonate is decomposed, we can use stoichiometry to calculate the mass of calcium oxide (CaO) produced.First, we need to convert the mass of calcium carbonate to moles using its molar mass:23.6 g CaCO3 / (100.09 g/mol) = 0.236 mol CaCO3Next, we use the stoichiometric relationship between calcium carbonate and calcium oxide, which is 1:1, to determine the moles of calcium oxide produced:0.236 mol CaCO3 × (1 mol CaO / 1 mol CaCO3) = 0.236 mol CaOFinally, we convert the moles of calcium oxide to grams using its molar mass:0.236 mol CaO × (56.08 g/mol) = 13.2 g CaOTherefore, the mass of calcium oxide produced from the decomposition of 23.6 g of calcium carbonate is 13.2 g.