I come to you in time of need, please help me get through this nightmare, help me solve problem 67? pretty please. 63. Consider the reaction between NiS₂ and O₂:→→→2 NiO(s) + 4 SO₂(g)2 NiS₂(s) + 5 O₂(g)When 11.2 g of NiS₂ react with 5.43 g of O₂, 4.86 g of NiO areobtained. Determine the limiting reactant, theoretical yieldof NiO, and percent yield for the reaction.65. Lead ions can be precipitated from solution with NaCl ac-cording to the reaction:PbCl₂(s) + 2 Na+ (aq)Pb²+ (aq) + 2 NaCl(aq)When 135.8 g of NaCl are added to a solution containing195.7 g of Pb²+, a PbCl₂ precipitate forms. The precipitateis filtered and dried and found to have a mass of 252.4 g.Determine the limiting reactant, theoretical yield of PbCl2,and percent yield for the reaction.67. Consider the reaction between TiO₂ and C:TiO2(s) + 2 C(s) →→→ Ti(s) + 2 CO(g)A reaction vessel initially contains 10.0 g of each of the reac-tants. Calculate the masses of TiO2, C, Ti, and CO that willbe in the reaction vessel after the reactants have reacted asmuch as possible. (Assume 100% yield.)ENTHALPY AND STOICHIOMETRY OF AHxn69. Classify each process as exothermic or endothermic and in-dicate the sign of AHrxn(a) butane gas burning in a lighter(c)(b) the reaction that occurs in the chemical cold packsused to ice athletic injuriesthe burning of wax in a candle66

#67: The balanced chemical equation is: TiO2(s) + 2C(s) ----> Ti(s) + 2CO(g) Moles of reactant…

67. Consider the reaction between TiO₂ and C: TiO₂ (s) + 2 C(s) → Ti(s) + 2 CO(g) A reaction vessel initially contains 10.0 g of each of the reac- tants. Calculate the masses of TiO2, C, Ti, and CO that will be in the reaction vessel after the reactants have reacted as much as possible. (Assume 100% yield.)

67. Consider the reaction between TiO₂ and C: TiO₂ (s) + 2 C(s) → Ti(s) + 2 CO(g) A reaction vessel initially contains 10.0 g of each of the reac- tants. Calculate the masses of TiO2, C, Ti, and CO that will be in the reaction vessel after the reactants have reacted as much as possible. (Assume 100% yield.)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 97E

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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.
4.8 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?
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
For this reaction, fill in the table with the indicated quantities for the balanced equation. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
4.37 The theoretical yield and the actual yield for various reactions are given below. Determine the corresponding percentage yields. Theoretical Yield Actual Yield Reaction 1 35.0 g 12.8 g Reaction 2 9.3 g 120 mg Reaction 3 3.7 metric tons 1250 kg Reaction 4 40.0 g 41.0 g
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.
list at least three quantities that must be conserved in chemical reactions.
A 0.20 mol sample of magnesium burns in air to form 0.20 mol of solid MgO. What amount (moles) of oxygen (O2) is required for a complete reaction?
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.
(a) Butane gas, C4H10, can burn completely in air [use O2(g) as the other reactant] to give carbon dioxide gas and water vapor. Write a balanced equation for this combustion reaction. (b) Write a balanced chemical equation for the complete combustion of C3H7BO3, a gasoline additive. The products of combustion are CO2(g), H2O(g), and B2O3(s).
In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.
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.

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