1. Write the balanced equation for the formation of lithium nitride from pure lithium metal and nitrogen gas. 6Li + N, 2Li,N Identify the limiting and excess reactants if 12.3 g of lithium are heated with 33.6 g of nitrogen gas. Calculate the theoretical yield of lithium nitride. Calculate the mass, in grams, of excess reactant. If 5.89 g of lithium nitride was formed during a run of this experiment, determine the percent yield.

1. Write the balanced equation for the formation of lithium nitride from pure lithium metal and nitrogen gas. 6Li + N, 2Li,N Identify the limiting and excess reactants if 12.3 g of lithium are heated with 33.6 g of nitrogen gas. Calculate the theoretical yield of lithium nitride. Calculate the mass, in grams, of excess reactant. If 5.89 g of lithium nitride was formed during a run of this experiment, determine the percent yield.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 51QAP: Write a balanced equation for (a) the combustion (reaction with oxygen gas) of glucose, C6H12O6, to...

See similar textbooks

Similar questions

Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
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.
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.
High cost and limited availability of a reactant often dictate which reactant is limiting in a particular process. Identify the limiting reactant when the reactions below are run, and come up with a reason to support your decision. a. Burning charcoal on a grill: C(s)+O2(g)CO2(g) b. Burning a chunk of Mg in water: Mg(s)+2H2O(l)Mg(OH)2(aq)+H2(g) c. The Haber process of ammonia production: 3H2(g)+N2(g)2NH3(g)
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)
Write a balanced equation for (a) the combustion (reaction with oxygen gas) of glucose, C6H12O6, to give carbon dioxide and water. (b) the reaction between xenon tetrafluoride gas and water to give xenon, oxygen, and hydrogen fluoride gases. (c) the reaction between aluminum and iron(III) oxide to give aluminum oxide and iron. (d) the formation of ammonia gas from its elements. (e) the reaction between sodium chloride, sulfur dioxide gas, steam, and oxygen to give sodium sulfate and hydrogen chloride gas.
4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
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.
Balance the following equations representing combustion reactions: a. b. c. C12H22O11 (s) + O2(g) CO2 (g) + H2O (g) d. Fe(s) + O2(g) Fe2O3(s) e. FeO(s) + O2(g) Fe2O3(s)