(Solved): Q1: DDT, an insecticide, is produced by the following reaction: chlorobenzene2C6H5Cl+ ...

Q1: DDT, an insecticide, is produced by the following reaction: $$\underset{\text{ chlorobenzene }}{2{\mathrm{C}}_6{\mathrm{H}}_5\mathrm{Cl}}+\underset{\text{ chloral }}{{\mathrm{C}}_2{\mathrm{HOCl}}_3}?\underset{\mathrm{DDT}}{{\mathrm{C}}_{14}{\mathrm{H}}_9{\mathrm{Cl}}_5}+{\mathrm{H}}_2\mathrm{O}$$ What mass of chloral is required to completely react with $$1142\mathrm{g}$$ of chlorobenzene? a) $$1495\mathrm{g}$$ b) $$747.7\mathrm{g}$$ c) $$147.4\mathrm{g}$$ d) $$571.0\mathrm{g}$$ Q2: Consider the following unbalanced equation: $${\mathrm{Ca}}_3{\left({\mathrm{PO}}_4\right)}_2(\mathrm{s})+{\mathrm{H}}_2{\mathrm{SO}}_4(\mathrm{aq})?{\mathrm{CaSO}}_4(\mathrm{s})+{\mathrm{H}}_3{\mathrm{PO}}_4(\mathrm{aq})$$ If $$1.0\mathrm{kg}$$ of calcium phosphate react with $$0.90\mathrm{kg}$$ of sulfuric acid, determine which reactant will be in excess and what mas will be leftover when the reaction is complete? a) sulfuric acid is in excess, $$0.58\mathrm{kg}$$ leftover b) sulfuric acid is in excess, $$6.0\mathrm{kg}$$ leftover c) calcium phosphate is in excess, $$0.051\mathrm{kg}$$ leftover d) calcium phosphate is in excess, $$0.166\mathrm{kg}$$ leftover Q3: Hydrogen peroxide can be prepared by the reaction of an acid with an alkaline earth metal peroxide, such as barium peroxide: $${\mathrm{BaO}}_2(\mathrm{s})+2\mathrm{HCl}(\mathrm{aq})?{\mathrm{H}}_2{\mathrm{O}}_2(\mathrm{aq})+{\mathrm{BaCl}}_2(\mathrm{aq})$$ What mass of hydrogen peroxide should result when $$1.50\mathrm{g}$$ of barium peroxide is treated with $$0.680\mathrm{g}$$ of hydrochloric acid? a) $$1.50\mathrm{g}$$ b) $$0.340\mathrm{g}$$ c) $$0.316\mathrm{g}$$ d) $$0.301\mathrm{g}$$ Q4: The industrial production of ammonia $$\left({\mathrm{NH}}_3\right)$$ involves reacting nitrogen gas with hydrogen gas. If $$18.2\mathrm{kg}$$ of ammonia is produced from a reaction mixture that contains $$6.0\mathrm{kg}$$ of hydrogen and $$30.0\mathrm{kg}$$ of nitrogen, what is the percent yield of the reaction? a) $$45.8\%$$ b) $$53.8\%$$ c) $$67.7\%$$ d) $$83.4\%$$ Q5: Consider the production of copper metal from copper ore: $$2{\mathrm{Cu}}_3{\mathrm{FeS}}_3(\mathrm{s})+7{\mathrm{O}}_2(\mathrm{g})?6\mathrm{Cu}(\mathrm{s})+2\mathrm{FeO}(\mathrm{s})+6{\mathrm{SO}}_2(\mathrm{g})$$ If $$2.50\mathrm{kg}$$ of copper ore ( $${\mathrm{Cu}}_3\mathrm{FeS}3$$ ) is reacted with $$0.60\mathrm{kg}$$ of oxygen gas and the process has an $$86.3\%$$ yield, what mass of pure copper is produced? a) $$1.05\mathrm{kg}$$ b) $$0.881\mathrm{kg}$$ c) $$0.677\mathrm{kg}$$ d) $$0.542\mathrm{kg}$$