Give the mayor product(s) of the following reaction. Brg (1 mole) ? heat Br Br Br Br Br Br I There is no reaction under these conditions or the correct product is not listed here.
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A: completely
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Q: The best balanced chemical equation for the complete combustion of: 1. hexane 2. nonane
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Q: how many moles of oxygen are required to burn 8.0 g of methane?
A: number of moles = mass/molar mass molar mass of CH4 = 16 g/mol
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Q: 3. Write a balanced equation of the combustion (with oxygen) of ethanol (C,H;OH).
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- 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.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.3.15 Ethanol, C2H5OH is found in gasoline blends used in many parts of North America. Write a balanced chemi- cal equation for the combustion of C2H5OH to form CO2 and HA.
- For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)Acetone, (CH3)2CO, is an important industrial compound. Although its toxicity is relatively low, workers using it must be careful to avoid flames and sparks because this compound burns readily in air. Write the balanced equation for the combustion of acetone.The Hall process is an important method by which pure aluminum is prepared from its oxide (alumina, Al2O3 ) by indirect reaction with graphite (carbon). Balance the following equation, which is a simplified representation of this process. m:math>Al2O3(s)+C(s)Al(s)+CO2(g)
- How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 0 atoms, 8 S atoms, and 14 N atoms?Consider the unbalanced equation for the combustion of propane: :math>C3H8(g)+O2(g)CO2(g)+H2O(g) rst, balance the equation. Then, for a given amount of propane, write the mole ratios that would enable you to calculate the number of moles of each product as well as the number of moles of O2that would be involved in a complete reaction. Finally, show how these mole ratios would be applied if 0.55 mole of propane is combusted.Answer these questions based on this reaction and the following information Mn(s) + 2 HCl(aq) ® MnCl2(aq) + H2(g) DH = -221 kJ 115.0 g of manganese is placed in a 1.25 L of a 3.50 M solution of hydrochloric acid. A. Which reactant is the limiting reagent? Show your work! B. How many moles of excess reagent are left over when the reaction is complete? Fill in the ICF chart to answer this question. Use mols from your earlier calculations to start filling in the ICF Chart Moles Excess Reagent Limiting Reagent Product Product 2 HCl Mn MnCl2 H2 Initial Mols Change in Mols Final Mols
- Complete combustion of propane (C3H8) produces carbon dioxide and water as products. C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g) Incomplete combustion produces some carbon monoxide (CO) in place of carbon dioxide (CO2). What is the limiting reactant for incomplete combustion? (A) There is no way to tell (B) Water (C) Propane (D) OxygenA lead ore, galena, consisting mainly of lead(II) sulfide, is the principal source of lead. To obtain the lead,the ore is first heated in the air to form lead oxide.PbS(s) + 3/2 O2(g) → Pb(s) + SO2 (g) ΔH = -415.4 kJThe oxide is then reduced to metal with carbon.PbO(s) + C(s) → Pb(s) + CO(g) ΔH = +108.5 kJCalculate ΔH for the reaction of one mole of lead(II) sulfide with oxygen and carbon, forming lead, sulfur dioxide, and carbon monoxide.If 20.0 mL of toluene (d=0.867 g/mL) is burned in air, how many grams of oxygen is needed for the complete combustion of the toluene?