) In Ammonia production, a reactor is supplied with a feed of 100 L of N2 and 400 L of H2 both at 22 atm and 420 °C. If the reaction is 95% complete (based on limiting reactant): a. Which is the limiting reactant? b. What is the number of moles of H2 remaining after the reaction? c. What is the number of moles of N2 remaining after the reaction? d. What is the % conversion of N2? e. What is the number of moles of NH3 after the reaction?

) In Ammonia production, a reactor is supplied with a feed of 100 L of N2 and 400 L of H2 both at 22 atm and 420 °C. If the reaction is 95% complete (based on limiting reactant): a. Which is the limiting reactant? b. What is the number of moles of H2 remaining after the reaction? c. What is the number of moles of N2 remaining after the reaction? d. What is the % conversion of N2? e. What is the number of moles of NH3 after the reaction?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.62PAE: 62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium...

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62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
Given the following reaction: 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(l) How many moles of water are produced when 3.0 moles of oxygen react? a. 2.6 mol H2O b. 90 mol H2O c. 0.089 mol H2O d. 2.0 mol H2O e. 333 mol H2O
4. How many moles of FeCl3 are produced from 2.3 grams of Fe? MW: Fe = 55.945g/mol, FeCl3 = 162.2g/mol' Fe + Cl2 -> FeCl3 SKR. 0.041 moles RKS. 0.082 moles KRS. 6.7 moles RSK. 0.021 moles
In Ammonia production, a reactor is supplied with a feed of 100L of N2 and 400L of H2 both at 22 atm and 420oC. If the reaction is 95% complete (base on limiting reactant):a. Which is the limiting reactant?b. What is the number of moles of H2 remaining after the reaction?c. What is the number of moles of N2 remaining after the reaction?d. What is the percent conversion of N2?e. What is the number of moles of NH3 after the reaction?
Combustion of hydrocarbon such as heptane produces carbon dioxide, a greenhouse gas. Greenhouse gases in the earths atmosphere can trap the suns heat, raising the average temperature of the earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. A. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid heptane into gaseous carbon dioxide and gaseous water. B. Suppose 0.260kg of heptane are burned in air at a pressure of exactly 1 atm and a temperature of 18°C. Calculate the volume of carbon dioxide that is produced in liters. Round your answer to three significant digits.
17. A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetraoxide (N2O4), which ignite on contact to form nitrogen gas and water vapor. How much in grams of the excess reagent is used up when 435.0 g of N2H4 and 718.5 g of N2O4 are mixed? (, MW: N204 = 92.011g/mol, N2H4 = 32.05g/mol, N2 =28.013 g/mol 2N2H4(0) + N2O40) –> 3N2(9) + 4H2O(g)
Gas Stoichiometry 1. Find the percent yield for the reaction of 1.56 gram BaCl2 when 1.86 gram of desired product of AgCl was isolated?
Given the following Reaction: 2C5H10O2 + 13O2 → 10CO2 + 10H2O. If 3.95 moles of O2 are reacted with an EXCESS of C5H10O21. a. a. How many moles of C5H10O2 are used? b. How many moles of H2O are produced? c. How many moles of C5H10O2 would you need to use to produce 4.42 moles of CO2 given that there is an excess of O2?
Given the following reaction : 5Fe+3O2 -> Fe3O4+2FeOSolve the following 4 sub-parts. a. How many moles of O2 are needed to react with 0.00382 mol of Fe?b. How many grams of FeO can be expected to form when 9.2 g of Fe react?c. How many moles of Fe3O4 will form when 0.559 g of FeO form?d. How many grams of FeO will form when 1.629 g of Fe react?
70 Nitrogen dioxide (NO2 gas and liquid water (H20) react to form aqueous nitric acid (HNO3) and nitrogen monoxide (NO) gas. Suppose you have 11.0 mo. of NO, and 13.0 mol of H20 in a reactor. 2 Suppose as much as possible of the NO, reacts. How much will be left? Round your answer to the nearest 0.1 mol. Imol x10 X Submit Assignment Continue woe ae Mook Po 04 pO DOD FA F12 esc F3 2 3 5 7 0 de T Y U P
10 moles of A reacts with 20 moles of B via the reaction A+B C+D The conversion of the limiting reactant is 75%. 1- Which reactant is the limiting? 2- What is the output number of moles of B?
Be sure to amswer all parts. The reaction between alumiaam and iron(lII) axide can generate temperatures approaching 3000°C and is used in welding metaks: 2A1 - Fe;O, - Al;O, +2Fe In one process, 146 g of Al are reacted with 601 g of Fe;O. Calculate the mass (in grams) of Alo, formed, and determine the amount of excess reagent left at the end of the reaction. mass of AlO, fermed: amount of excess reagent left:

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