Ammonia (NH,) gas and oxygen (O₂) gas react to form nitrogen (N₂) gas and water (H₂O) vapor. Suppose you have 5.0 mol of NH, and 13.0 mol of O, in a reactor. Suppose as much as possible of the NH, reacts. How much will be left? Round your answer to the nearest 0.1 mol. X

Ammonia (NH,) gas and oxygen (O₂) gas react to form nitrogen (N₂) gas and water (H₂O) vapor. Suppose you have 5.0 mol of NH, and 13.0 mol of O, in a reactor. Suppose as much as possible of the NH, reacts. How much will be left? Round your answer to the nearest 0.1 mol. X

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 54A

See similar textbooks

Similar questions

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?
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.
Magnesium ribbon reacts with acid to produce hydro- gen gas and magnesium ions. Different masses of magnesium ribbon are added to 10 mL of the acid. The volume of the hydrogen gas obtained is a measure of the number of moles of hydrogen produced by the reaction. Various measurements are given in the table below. (a) Draw a graph of the results by plotting the mass of Mg versus the volume of the hydrogen gas. (b) What is the limiting reactant in experiment 1? (c) What is the limiting reactant in experiment 3? (d) What is the limiting reactant in experiment 6? (e) Which experiment uses stoichiometric amounts of each reactant? (f) What volume of gas would be obtained if 0.300 g of Mg ribbon were used? If 0.010 g were used?
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.
Alkali metal hydroxides are sometimes used to “scrub” excess carbon dioxide from the air in closed spaces (such as submarines and spacecraft). For example, lithium hydroxide reacts with carbon dioxide according to the unbalanced chemical equation :math>LiOH(s)+CO2(g)Li2CO3(s)+H2O(g) ppose a lithium hydroxide canister contains 155 g of LiOH(s). What mass of CO2(g)will the canister be able to absorb? If it is found that after 24 hours of use the canister has absorbed 102 g of carbon dioxide, what percentage of its capacity has been reached?
3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of operation. How many moles of NO2 would this engine release if it were used for a 45-minute commute, assuming that this mea- sured number is representative of the emission under all circumstances?
Electrolysis Determine the theoretical and percent yield of hydrogen gas if 36.0 g ofwater undergoes electrolysis to produce hydrogen and oxygen and 3.80 g of hydrogen is collected.
Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.
Iron reacts with oxygen as Shown. 4Fe(s)+3O2(g)2FeO3(s) Different amounts of iron were burned in a fixed amount of oxygen. For each mass of iron burned, the mass Of iron(lll) oxide formed was plotted on the graph shown Figure 11.15. Why does the graph level off after 25.0 g of iron is burned? How many moles of oxygen are present in the fixed amount?
When aluminum is mixed with iron(lll) oxide, iron metal and aluminum oxide are produced, along with a large quantity of heat. What mole ratio would you use to determine moles of Fe if moles of Fe2O3 is known? Fe2O3(s)+2A1(s)2Fe(s)+A12O3(s)+heat
Calculate the number of moles of CO2 generated by the reaction of Exercise 5.42 when 500.g of CaO is produced.

SEE MORE QUESTIONS

Recommended textbooks for you

World of Chemistry

Chemistry

ISBN:

9780618562763

Author:

Steven S. Zumdahl

Publisher:

Houghton Mifflin College Div

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

World of Chemistry

Chemistry

ISBN:

9780618562763

Author:

Steven S. Zumdahl

Publisher:

Houghton Mifflin College Div

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS