Dissolving 3.00 g of an impure Sam apple of calcium carbonate in hydrochloric acid produced .656 L of carbon dioxide at 20.0 °C and 792 mmHg.
CaCO3 (s) + 2HCL (aq) —> CaCl2 (aq) + CO2 (g) + H2O (l)
Calculate the percent by mass of calcium carbonate in the original sample, assuming that the impurities do not react with HCL.
%CaCO3
Your answer should be rounded to three significant digits
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There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. in the first step, calcium carbide and water react to form acetylene and calcium hydroxide: cac2 (s) + 2h2o (g) → c2h2 (g) + caoh2 (s) =δh−414.kj in the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6c2h2 (g) + 3co2 (g) + 4h2o (g) → 5ch2chco2h (g) =δh132.kj calculate the net change in enthalpy for the formation of one mole of acrylic acid from calcium carbide, water and carbon dioxide from these reactions. round your answer to the nearest kj .
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Dissolving 3.00 g of an impure Sam apple of calcium carbonate in hydrochloric acid produced .656 L o...
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