7. How many moles of O₂ react with or are produced by 5.67 moles of the first reactant shown in eachbalancedequation?4CO2 + 6H₂Oa.b.C.b.C.b.C.d.e.2C2H6 + 7022KCIO38. How many grams of the second reactant is needed to react with 18.3 grams of the first reactant in eachbalanced equation?a.4Fe + 30₂29 c.9 d.9 e.a.P4 + 6C1₂b.P4O10+ 6H2O2KC1+30₂203 + 3COP4O10+ 6H2O9 a.9 b.→2Fe₂O39. Using the balanced equations below, complete 9.a through 9.d:a.4PC134H3PO4How many grams of the first product can be produced from 15.0 grams of the first reactant2Fe + 3CO2and 15.0 grams of the second reactant?Which reactant is the limiting reactant?Which reactant is the excess reactant?4H3PO4How many grams of the excess reactant are reacted?How many grams of the excess reactant are left unreacted?10. A student carried out the reaction shown by reacting 7.38g P4 with excess Cl₂ and obtained 35.0g ofPC13.P4 + 6Cl24PCL3What is the theoretical yield of PC13?Calculate the % yield of PC13.

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7. How many moles of O₂ react with or are produced by 5.67 moles of the first reactant shown in each balanced equation? a. 2C₂H6 + 702 4CO2 + 6H₂O 8 b. C. 2KC103 4Fe +302- 2KC1 + 30₂ →2Fe₂O3 How many grams of the second reactant is needed to react with 18.3 grams of the first reactant in each

7. How many moles of O₂ react with or are produced by 5.67 moles of the first reactant shown in each balanced equation? a. 2C₂H6 + 702 4CO2 + 6H₂O 8 b. C. 2KC103 4Fe +302- 2KC1 + 30₂ →2Fe₂O3 How many grams of the second reactant is needed to react with 18.3 grams of the first reactant in each

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 66QAP: Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine...

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Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine and 3.68 mol of fluorine are combined. (Assume 100% yield for the reaction.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of chlorine trifluoride in moles? (d) How many moles of excess reactant remain after reaction is complete.
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.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. C2N2(g)+7F2(g)2CF4(g)+2NF3(g)(a) How many moles of fluorine react with 1.37 mol of cyanogen? (b) How many moles of CF4 are obtained from 13.75 mol of fluorine? (c) How many moles of cyanogen are required to produce 0.8974 mol of NF3? (d) How many moles of fluorine will yield 4.981 mol of nitrogen trifluoride?
For each of the following balanced reactions, calculate how many moles of each product would be produced by complete conversion of 0.50 mole of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;2H2O(l)2H2O(l)+O2(g) msp;2KClO3(s)2KCl(s)+3O2(g) msp;2Al(s)+6HCl(aq)2AlCl3(aq)+3H2(g) msp;C3H8(g)+5O2(g)3CO2(g)+4H2O(g)
For each of the following balanced chemical equations, calculate how many moles of product(s) would be produced if 0.500 mole of the first reactant were lo react completely. msp;CO2(g)+4H2(g)CH4(g)+2H2O(l) msp;BaCl2(aq)+2AgNO3(aq)2AgCl(s)+Ba(NO3)2(aq) msp;C3H8(g)+5O2(g)4H2O(l)+3CO2(g) msp;3H2SO4(aq)+2Fe(s)Fe2(SO4)3(aq)+3H2(g)
Ammonia reacts with a limited amount of oxygen according to the equation 4NH3(g)+5O2(g)4NO(g)+6H2O(l)(a) How many moles of NO are obtained when 3.914 moles of oxygen are used? (b) How many moles of oxygen are required to react with 2.611 moles of ammonia? (c) How many moles of water are obtained when 0.8144 moles of ammonia are used? (d) How many moles of oxygen are required to produce 0.2179 mol of water?
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)
For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0. 145 mole of the first reactant. msp;BaCl2(aq)+H2SO4(aq) msp;AgNO3(aq)+NaCl(aq) msp;Pb(NO3)2(aq)+Na2CO3(aq) msp;C3H8(g)+O2(g)
Sand is mainly silicon dioxide. When sand is heated with an excess of coke (carbon), pure silicon and carbon monoxide are produced. (a) Write a balanced equation for the reaction. (b) How many moles of silicon dioxide are required to form 20.00 g of silicon? (c) How many grams of carbon monoxide are formed when 98.76 g of silicon are produced?
The gaseous hydrocarbon acetylene, C2H2, is used in welders’ torches because of the large amount of heat released when acetylene burns with oxygen. :math>2C2H2(g)+5O2(g)4CO2(g)+2H2O(g) w many grams of oxygen gas are needed for the complete combustion of 150 g of acetylene?
For each of the following balanced chemical equations, calculate how many grams of the product(s) would be produced by complete reaction of 0.125 mole of the first reactant. msp;AgNO3(aq)+LiOH(aq)AgOH(s)+LiNO3(aq) msp;Al2(SO4)3(aq)+3CaCl2(aq)2AlCl3(aq)+3CaSO4(s) msp;CaCO3(s)+2HCl(aq)CaCl2(aq)+CO2(g)+H2O(l) msp;2C4H10(g)+13O2(g)8CO2(g)+10H2O(g)