Set up and answer with options below STARTING AMOUNTXConsider the reaction of solid PbO and gaseous NH3 to form solid Pb, nitrogengas, and water vapor.The balanced chemical equation is 3 PbO(s) + 2 NH3(g)How many grams of N₂ will be produced from 0.447chemical equation?28.02ADD FACTOR* ( )223.214.014.17DELETEf0.4470.0479g N₂/mol N₂ g PbO/mol PbO g N₂99.82.09ANSWERmol PbO3 Pb(s) + N₂(g) + 3 H₂O(g).moles of PbO balanced93212.5g PbO3RESETmol N₂1

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Consider the reaction of solid PbO and gaseous NH, to form solid Pb, nitrogen gas, and water vapor. The balanced chemical equation is 3 PbO(s) + 2 NH₂(g) How many grams of N₂ will be produced from 0.447 chemical equation? 3 Pb(s) + N₂(g) + 3 H₂O(g). moles of PbO balanced

Consider the reaction of solid PbO and gaseous NH, to form solid Pb, nitrogen gas, and water vapor. The balanced chemical equation is 3 PbO(s) + 2 NH₂(g) How many grams of N₂ will be produced from 0.447 chemical equation? 3 Pb(s) + N₂(g) + 3 H₂O(g). moles of PbO balanced

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 7QAP

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Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.
For each of the following unbalanced chemical equations, suppose exactly 5.0 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, assuming that the limiting reactant is completely consumed. msp;Na(s)+Br2(l)NaBr(s) msp;Zn(s)+CuSO4(aq)ZnSO4(aq)+Cu(s) msp;NH4Cl(aq)+NaOH(aq)NH3(g)+H2O(l)+NaCl(aq) msp;Fe2O3(s)+CO(g)Fe(s)+CO2(g)
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A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?
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)
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Although many sulfate salts are soluble in water, calcium sulfate is not (Table 7. 1). Therefore, a solution of calcium chloride will react with sodium sulfate solution to produce a precipitate of calcium sulfate. The balanced equation is :math>CaCl2(aq)+Na2SO4(aq)CaSO4(s)+2NaCl(aq) a solution containing 5.21 g of calcium chloride is combined with a solution containing 4.95 g of sodium sulfate, which is the limiting reactant? Which reactant is present in excess?
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he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.