Ammonia (NH,) gas and oxygen (0,) gas react to form nitrogen (N,) gas and water (H,0) vapor. Suppose you have 1.0 mol of NH, and 2.0 mol of O, in a reactor. Could half the NH, react? O yes O no If you answered yes, calculate how many moles of N, would be produced. Round your answer to the nearest 0.1 mol. O mol

Ammonia (NH,) gas and oxygen (0,) gas react to form nitrogen (N,) gas and water (H,0) vapor. Suppose you have 1.0 mol of NH, and 2.0 mol of O, in a reactor. Could half the NH, react? O yes O no If you answered yes, calculate how many moles of N, would be produced. Round your answer to the nearest 0.1 mol. O mol

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 9QAP: onsider the balanced chemical equation :math>4Al(s)+3O2(g)2Al2O3(s). at mole ratio would you use to...

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Sodium borate decahydrate, Na2B4O710H2O is commonly known as borax. It is used as a deodorizer and mold inhibitor. A sample weighing 15.86 g is heated until a constant mass is obtained indicating that all the water has been evaporated off. (a) What percent, by mass of Na2B4O710H2O is water? (b) What is the mass of the anhydrous sodium borate, Na2B4O7?
An air bag is deployed by utilizing the following re tion the nitrogen gas produced inflates the air bag): :math>2NaN3(s)2Na(s)+3N2(g) 10.5 g of NaN1 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, what is the percent yield?
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?
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
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?
Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. l type='a'> Write the balanced equation for the reaction that is (occurring. including all phases. If a 100.0-g sample of calcium carbide (CaC2)is initially reacted with 50.0 g of water, which reactant is limiting? Prove that mass is conserved for the reactant amounts used in pan b.
When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. :math>C(s)+O2(g)CO2(g) wever, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. :math>2C(s)+O2(g)CO(g) at mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?
The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.
When 9.59 g of a certain vanadium oxide is heated in the presence of hydrogen, and a new oxide of vanadium are formed. This new vanadium oxide has a mass of 8.76 g. When the second vanadium oxide undergoes additional heating in the presence Of hydrogen, 5.38 g of vanadium metal forms, a. Determine the empirical formulas for the two vanadium oxides. b. Write balanced equations for the Steps of the reaction. c. Determine the mass of hydrogen needed to complete the steps of this reaction.
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.
When small quantities of elemental hydrogen gas are needed for laboratory work, the hydrogen is often generated by chemical reaction of a metal with acid. For example, tine reacts with hydrochloric acid, releasing gaseous elemental hydrogen: :math>Zn(s)+2HCI(aq)ZnCl2(aq)+H2(g) at mass of hydrogen gas is produced when 2.50 g of zinc is reacted with excess aqueous hydrochloride acid?
Atoms of three different elements are represented by O, , and . Which compound is left over when three molecules of O. and three molecules of . react to form O. And O?