If 1.00 g mixture of CaCl2 and Na,CO3 are put in a beaker and 100 mL of warm water is added and heated for 10 minutes. The precipitated product that formed in the reaction is CaCO3. If the mass of the product formed is 0.361 g and Na,CO3 is the limiting reactant, what is the mass percent of Na,CO3 in the mixture? (The atomic mass of Na 23, C = 12.0, O = 16.0, Ca 40.1 and Cl = 35.45 g/mol)

If 1.00 g mixture of CaCl2 and Na,CO3 are put in a beaker and 100 mL of warm water is added and heated for 10 minutes. The precipitated product that formed in the reaction is CaCO3. If the mass of the product formed is 0.361 g and Na,CO3 is the limiting reactant, what is the mass percent of Na,CO3 in the mixture? (The atomic mass of Na 23, C = 12.0, O = 16.0, Ca 40.1 and Cl = 35.45 g/mol)

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ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

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A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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