T Normal T No Spac. Heading 1Heading 2TitleFontParagraphStyles1. Number of oxygen molecules reacting with (68g) ammonia according to thefollowing equation:4NH3 + 502 -4 NO+ 6 HLOIs:a) 1.9 x 1024b) 1.2 x 1024c) 9.5 x 1024d) 3.0 x 1024.2) For the following reaction:N2 (g) + 3H2 (g) →2NH3 (g)The mass of NH3 resulting from the reaction 0.25mol of H2 is:a) 4.25gb) 1.33gc) 6.38gd) 2.83g3) If 1.2 mol of phosphorus (P) interacts with 1.2 mol of chlorine according to thefollowing equation:2P + 3Cl2 → 2 PCl3The limiting substance of the reaction:a) Cl2b) Pc) PCI3d) Not one.36°Chpf516f7f8f9f10f11f12insertसलाdele&backspace6 7809.

Given reaction is : 4NH3 + 5O2 --------------> 4NO + 6H2O Given mass of NH3 = 68 g Gram molar…

Answered: Styles 1. Number of oxygen molecules…

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter4: Chemical Reactions

Section: Chapter Questions

Problem 4.19P

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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ookmarks Profiles Tab Window Help G molar r ste X Learnir O Checko R Search M Ryerso E Ryerso Jassignments/389/tasks/103 The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in the presence of a catalyst to produce ammonia. It is currently the main industrial source of ammonia. N2 (g) + 3 H2 (g) 2 NH3 (g) Assuming that a reaction vessel originally contains 0.400 moles of N, and 0.900 moles of H2 , answer each of the following questions: a) How many moles of NH3 could be produced from these quantities of N, and H2 ? mol NH3 0.600 b) After the reaction is complete, how many moles of N2 would remain? mol N2 0.100 c) After the reaction is complete, how many moles of H2 would remain? moles H2 0.8

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Styles 1. Number of oxygen molecules reacting with (68g) ammonia according to the following equation: 4NH3 + 502 -4 NO + 6 H0 Is: a) 1.9 x 1024 b) 1.2 x 1024 c) 9.5 x 1024 d) 3.0 x 1024.