TZodutoe Mc 4.1 For each of the following balanced equations, calculate the mass of the second reactant needed to completely react with 100 ge of the first reactant. (a) 2 K(s) +2H2O(g)2 KOH(aq) +H2(g) O (b) 2 Al(s) +3 F2(g)2 AIF3(s) rvis USA (c) 4NH3(g)+5 O2(g) 4NO(g) +6 H2O(g) t(d) Fe2O3(s) +3C(s)2 Fe(l) +3 CO(g) (e) CaC2(s) +2H20(I)Ca(OH)2 (s) +C2H2(g) (f) SiO2(s) +4 HF (g) SiF4(g) + 2 H2O(I) 10 aph (g) 2C4H10(g) + 13 O2 (g)8 CO2(g) + 10 H2O(g) nsuo (h) BaCl2 (aq) + Na2SO4 (aq)2 NaCl(aq) + BaSO4 (s) 4.2 Given 100.0 g of each reactant in the reactions described by the Osl preceding equations, which reactant is the limiting reactant, and what mass of the first product listed will be formed? Mot 7OULS ikG gs 83

TZodutoe Mc 4.1 For each of the following balanced equations, calculate the mass of the second reactant needed to completely react with 100 ge of the first reactant. (a) 2 K(s) +2H2O(g)2 KOH(aq) +H2(g) O (b) 2 Al(s) +3 F2(g)2 AIF3(s) rvis USA (c) 4NH3(g)+5 O2(g) 4NO(g) +6 H2O(g) t(d) Fe2O3(s) +3C(s)2 Fe(l) +3 CO(g) (e) CaC2(s) +2H20(I)Ca(OH)2 (s) +C2H2(g) (f) SiO2(s) +4 HF (g) SiF4(g) + 2 H2O(I) 10 aph (g) 2C4H10(g) + 13 O2 (g)8 CO2(g) + 10 H2O(g) nsuo (h) BaCl2 (aq) + Na2SO4 (aq)2 NaCl(aq) + BaSO4 (s) 4.2 Given 100.0 g of each reactant in the reactions described by the Osl preceding equations, which reactant is the limiting reactant, and what mass of the first product listed will be formed? Mot 7OULS ikG gs 83

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.77PAE: The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce...

See similar textbooks

Similar questions

Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
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. D 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.
4.42 Sulfur hexafluoride is a very stable gas useful ¡n electrical generators and switches. It is formed by direct synthesis from the elements: S(s)+3F2(g)SF6(g) If 92 g of SF6 is produced from the reaction of 115 g of sulfur ¡n excess fluorine, what is the percentage yield? Sulfur hexafluoride, SF6
4-93 Ammonia is prepared industrially by the reaction of nitrogen and hydrogen according to the following equation: If 29.7 kg of N2 is added to 3.31 kg of H2, (a) Which reactant is the limiting reagent? (b) How many grams of the other reactant are left over? (c) How many grams of NH3 are formed if the reaction goes to completion?
Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
3.93 Adipic acid is used in the production of nylon, so it is manufactured in large quantities. The most common method for the preparation of adipic acid is the reaction of cyclohexane with oxygen. Balance the skeleton equation shown be1ow.
Cisplatin [Pt(NH3)2Cl2], an anticancer agent used for the treatment of solid tumors, is prepared by the reaction of ammonia (NH3) with potassium tetrachloroplatinate (K2PtCl4). Assume that 10.0 g of K2PtCl4 and 10.0 g of NH3 are allowed to react.K2PtCl4 + 2 NH3  Pt(NH3)2Cl2 + 2 KCla) Which reactant is limiting, and which is in excess?b) How many grams of the excess reactant are consumed, and how many grams remain?c) How many grams of cisplatin are formed?
Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 63.5% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 70000 kg coal that is 0.44 mass % sulfur?
Coal Combustion -- Limestone for SO2 Scrubbing Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 70.5% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 69000 kg coal that is 0.42 mass % sulfur?
Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: Ca + V2O5 --> CaO + V In one process, 1.54x 103 g of V2O5 (MM = 181.88g/mol) react with 1.96 x103 g of Ca. (MM = 40.08g/mol) (1) Determine the limiting reactant. (2) Determine the excess reactant. (3) Calculate the theoretical yield of V. (MM = 50.94g/mol) (4) Calculate the percent yield if 803 g of V are actually obtained.
Solid diiodine pentoxide is used in respirators to remove carbon monoxide from air. The reaction producessolid iodine and carbon dioxide gas.a. What mass of carbon monoxide could be removed from air by a respirator that contains 5.0 g of diiodinepentoxide?b. What mass of iodine would remain in the respirator?