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

The correct answer is 132 g of calcium oxide.<br /><br />Explanation:<br />The balanced chemical equation for the decomposition of calcium carbonate (CaCO3) is:<br /><br />CaCO3(s) → CaO(s) + CO2(g)<br /><br />Given that 23.6 g of calcium carbonate is decomposed, we can use stoichiometry to calculate the mass of calcium oxide (CaO) produced.<br /><br />First, we need to convert the mass of calcium carbonate to moles using its molar mass:<br />23.6 g CaCO3 / (100.09 g/mol) = 0.236 mol CaCO3<br /><br />Next, we use the stoichiometric relationship between calcium carbonate and calcium oxide, which is 1:1, to determine the moles of calcium oxide produced:<br />0.236 mol CaCO3 × (1 mol CaO / 1 mol CaCO3) = 0.236 mol CaO<br /><br />Finally, we convert the moles of calcium oxide to grams using its molar mass:<br />0.236 mol CaO × (56.08 g/mol) = 13.2 g CaO<br /><br />Therefore, the mass of calcium oxide produced from the decomposition of 23.6 g of calcium carbonate is 13.2 g.