886 mol NO 2 c O 2 is the reactant left over with the amount of 0503 0443 006

886 mol no 2 c o 2 is the reactant left over with the

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2c) O2is the reactant left over with the amount of0.503 – 0.443 = 0.06 mol O28Propane (C3H8) is a component of natural gas and is used in domestic cooking and heating. It burns according to the following reaction:C3H8+ O2CO2+ H2OaBalance the equation representing the combustion of propane in air. (5 points)bHow many grams of carbon dioxide can be produced by burning 20.0 pounds of propane, the typical size of a BBG grill propane tank? Assume that oxygen is the excess reagent in this reaction. (5 points)aC3H8+ 5O23CO2+ 4H2ObO2 is the excess reagent → propane is the limiting reagentC3H8+ 5O23CO2+ 4H2O44 g 132 g 20 lbs C3H8 = 20 / 2.2 = 9.09 kg C3H89.09 kg (9.09 x 132) / 44 = 27.27 = 27 kg CO29Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reactionCaF2+ H2SO4CaSO4+ 2HFIn one process 6.00 kg of CaF2are treated with an excess of H2SO4and yield 2.86 kg of HF. Calculate the percent yield of HF. (5 points)(Reference: Chang 3.89)CaF2+ H2SO4CaSO4+ 2HF78.1g 40gTheoretical yield of HF = (6.00 x 40) / 78.1 = 3.07 = 3.1 kg HF% yield of HF = (2.86 / 3.1) x 100% = 92%10Certain race cars use methanol (CH3OH; also called wood alcohol) as a fuel. Methanol has amolecular mass of 32.0 g/mol and a density of 0.79 g/mL. The combustion of methanol occurs according to the following equation:
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2CH3OH + 3O22CO2+ 4H2OIn a particular reaction 2.00 L of methanol are reacted with 80.0 kg of oxygen.
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