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- A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
- Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.Decane, C10H22(l), undergoes complete combustion if there is sufficient oxygen available: 2 C10H22(l) + 31 O2(g) → 20 CO2(g) + 22 H2O(g) (a) What mass of oxygen is required for the complete combustion of 800g of decane? (b) A sample of decane is burned, producing 12 mol of carbon dioxide. What amount (moles) of water is also produced? Include a therefore statement for EACH a) and b)The following is the balanced equation for the combustion of butanol in oxygen:C4H9OH(g) + 6O2 --> 4 NO(g) + 6H2O(g) a. How many grams of butanol must be burned to produce 18.50g of carbon dioxide? b. How many grams of water are also produced? c. How many grams of oxygen are needed to produce 18.50g of carbon dioxide? d. Use the results from a, b and c to show this reaction obeys the law of conservation of mass.
- Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.634 °C. What quantity in moles of C₅H₈ were burned?The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18)(C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 4.2 kgkg of octane burned. ( HintHint: Begin by writing a balanced equation for the combustion reaction.)Given the combustion reaction below how many moles of CO2 are formed given that you start with 1.50×10^-2 mol of C3H8O
- In 1997, at the United Nations Conference on Climate Change, the major industrial nations agreed to expand their re-search efforts to develop renewable sources of carbon-basedfuels. For more than a decade, Brazil has been engaged in aprogram to replace gasoline with ethanol derived from the rootcrop manioc (cassava).(a) Write separate balanced equations for the complete combus-tion of ethanol (C₂H₅OH) and of gasoline (represented by theformula C₈H₁₈).(b) What mass of oxygen is required to burn completely 1.00 Lof a mixture that is 90.0% gasoline (d=0.742 g/mL) and 10.0%ethanol (d=0.789 g/mL) by volume?(c) If 1.00 mol of O₂ occupies 22.4 L, what volume of O₂ isneeded to burn 1.00 L of the mixture?(d) Air is 20.9% O₂ by volume. What volume of air is needed toburn 1.00 L of the mixture?Glucose (CH1206) is combusted under an excess of pure oxygen. This reaction produces 20.0g of COz(g). a) Write out and balance the combustion reaction. b) How much glucose (in g) was there to begin with? c) What mass of O2 would be required to burn 25.0g of glucose?Consider this given balanced reaction for the combustion of propane: C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4 H2O(g) If I gave you moles of C3H8 and wanted you to calculate moles of steam, which mole ratio would you use? a) (5 mol O2 / 1 mol C3H8) b) (1 mol C3H8 / 5 mol O2 ) c) (4 mol H2O / 5 mol O2) d) (4 mol H2O / 1 mol C3H8) e) (1 mol C3H8 / 4 mol H2O)