13 1Amount =56Use the References to access important values if needed for this question.According to the following reaction, how many moles of oxygen gas are necessary to form 0.963 moles carbon dioxide?carbon monoxide(g) + oxygen(g) → carbon dioxide(g)RFSubmit Answer%5TGmolRetry Entire Group 9 more group attempts remaining6MacBook AirF6YHment-take&7U*8AFB(9KF9O0dF10PUWLv2 | Online teaching and X-F11Previous+11[Next>7Save and ExitF12D8Bdelete According to the following reaction, how many moles of ethane (C₂H6) will be formed upon the complete reaction of 0.737 moleshydrogen gas with excess ethylene (C₂H4)?hydrogen (g) + ethylene (C₂H4) (g)-ethane (C₂H6) (g)moles ethane (C₂H6)e 2$RSubmit AnswerFF4965TGBRetry Entire Group6Use thYHtv Sferences to access important values if needed for this question.N&79 more group attempts remainingMacBook AirwwwUFZJ8MA1D-HIK(9XVSDDO)OLloP:2¡?{[Previous?DA+1Next>Save and ExitF121deleteO O 1?

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7 Use the References to access important values if needed for this question. According to the following reaction, how many moles of oxygen gas are necessary to form 0.963 moles carbon dioxide? carbon monoxide(g) + oxygen(g) → carbon dioxide (g) mol Amount = A R Submit Answer 888 % 5 T Retry Entire Group 9 more group attempts remaining 6 MacBook Air Y TAO - 7 U 8 DII ( 9 DD FO O ) O lo F10 P Previous AL F11 { + [ = Next> Save and Exit 642 delete 1 1

7 Use the References to access important values if needed for this question. According to the following reaction, how many moles of oxygen gas are necessary to form 0.963 moles carbon dioxide? carbon monoxide(g) + oxygen(g) → carbon dioxide (g) mol Amount = A R Submit Answer 888 % 5 T Retry Entire Group 9 more group attempts remaining 6 MacBook Air Y TAO - 7 U 8 DII ( 9 DD FO O ) O lo F10 P Previous AL F11 { + [ = Next> Save and Exit 642 delete 1 1

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 6QAP: or each of the following reactions, give the balanced chemical equation for the reaction and state...

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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)
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.
or each of the following reactions, give the balanced chemical equation for the reaction and state the meaning of the equation in terms of individual molecules and in terms of moles of molecules. msp;MnO2(s)+Al(s)Mn(s)+Al2O3(s) msp;B2O3(s)+CaF2(s)BF3(g)+CaO(s) msp;NO2(g)+H2O(l)HNO3(aq)+NO(g) msp;C6H2(g)+H2C6(g)H12(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)
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 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)
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)
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?
Consider the following generic reaction: Y2+2XY2XY2 In a limiting reactant problem, a certain quantity of each reactant is given and you are usually asked to calculate the mass of product formed. If 10.0 g of Y2 is reacted with 10.0 g of XY, outline two methods you could use to determine which reactant is limiting (runs out first) and thus determines the mass of product formed.
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?
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.