Although xenon is a "noble gas," it reacts with fluorine and oxygen. When xenon gas reacts with F2 gas, XeF4 is one of the products. If 47.8 g of xenon reacts with excess fluorine and generates 38.2 g of XeF4, what is the percent yield and how much xenon remains unreacted, assuming no other product forms? % yield g xenon remains unreacted

Although xenon is a "noble gas," it reacts with fluorine and oxygen. When xenon gas reacts with F2 gas, XeF4 is one of the products. If 47.8 g of xenon reacts with excess fluorine and generates 38.2 g of XeF4, what is the percent yield and how much xenon remains unreacted, assuming no other product forms? % yield g xenon remains unreacted

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter11: Stoichiometry

Section: Chapter Questions

Problem 90A

See similar textbooks

Similar questions

Cryolite (Na3AlF6) is used in the production of aluminumfrom its ores. It is made by the reaction 6NaOH+Al2O3+12HF2Na3AlF6+9H2O Calculate the mass of cryolite that can be prepared by thecomplete reaction of 287gAl2O3 .
onsider the balanced chemical equation :math>4Al(s)+3O2(g)2Al2O3(s). at mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely?
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.
At high temperatures, silicon dioxide reacts with carbon to produce silicon carbide, SiC, also known as carborundum, an important industrial abrasive. If the reaction is run with 100. g of each reactant: (a) Determine the limiting reactant; and (b) Calculate the mass of excess reactant remaining after the reaction is over.
Air Pollution Nitrogen monoxide, which is present in urban air pollution, immediately Converts to nitrogen dioxide as it reacts with oxygen. a. Write the balanced chemical equation for the formation of nitrogen dioxide from nitrogen monoxide. b. What mole ratio would you use to convert from moles of nitrogen monoxide to moles of nitrogen dioxide?
Billions of pounds of urea, CO(NH2)2, are produced annually for use as a fertilizer. The principal reaction employed is: 2NH3+CO2CO(NH2)2+H2O By assuming unlimited amounts of CO2, how many moles of urea can be produced from each of the following amounts of NH3? a.2molNH3b.0.45molNH3c.10gNH3d.2.0kgNH3