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 (CaC) and water react to form acetylene (C,H,) and calcium hydroxide: CaC (s) + 2H,0(g) C,H,(g) + Ca(OH),(9) In the second step, acetylene (C,H), carbon dioxide and water react to form acrylic acid (CH,CHCO,H): 6C,H,(g) + 3 CO2(g) + 4H,0(g) 5 CH,CHCO,H(g) Suppose the yield of the first step is 96.% and the yield of the second step is 79.%. Calculate the mass of calcium carbide required to make 2.0 kg of acrylic acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.

The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3Al(s)+3NH4ClO4(s)Al2O3(s)+AlCl3(s)+3NO(g)+6H2O(g) Calculate H for this reaction

Consider the two space shuttle fuel reactions in Exercises 81 and 82. Which reaction produces more energy per kilogram of reactant mixture (stoichiometric amounts)? 81. The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3Al(s)+3NH4ClO4(s)Al2O3(s)+AlCl3(s)+3NO(g)+6H2O(g) Calculate H for this reaction 82. The space shuttle Orbiter utilizes the oxidation of methylhydrazine by dinitrogen tetroxide for propulsion: 4N2H3CH3(l)+5N2O4(l)12H2O(g)+9N2(g)+4CO2(g) Calculate H for this reaction

Consider the reaction 2ClF3(g)+2NH3(g)N2(g)+6HF(g)+Cl2(g)H=1196KJ Calculate H for CIF3(g).

Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.

Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.

Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.

4.60 Why are fuel additives used?

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 (CaC,) and water react to form acetylene (C,H,) and calcium hydroxide: CaC, (s) + 2H,0(g) - C,H,(g) + Ca(OH), (s) In the second step, acetylene (C,H,), carbon dioxide and water react to form acrylic acid (CH,CHCO,H): 6C,H, (g) 3co,(g) + 4H,0(g) 5 CH, CHCO,H (g) Suppose the yield of the first step is 68.% and the yield of the second step is 66.%. Calculate the mass of calcium carbide required to make 10.0 kg of acrylic acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: Na(g) + 3H,(g) – 2NH;(g) In the second step, ammonia and oxygen react to form nitric acid (HNO) and water: NH,(g) + 20,(g) HNO-(g) + H,0(g) Suppose the yield of the first step is 70.% and the yield of the second step is 61.%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits.