Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process.In the first step, nitrogen and hydrogen react to form ammonia:N2(g)+3 H,(g)→2 NH3(g)圖In the second step, ammonia and oxygen react to form nitric acid and water:NH, (g)+20,(g)–HNO;(g)+H,0(g)oloWrite the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.

Given two steps for the manufacturing of HNO3 is : Step.1 :- N2 (g) + 3H2 (g) --------> 2NH3 (g)…

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N3(g)+3 H,(g) 2NH,(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH,(g)+20,(g)-HNO3(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced. D-D On O

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N3(g)+3 H,(g) 2NH,(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH,(g)+20,(g)-HNO3(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced. D-D On O

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Aspirin (C9H8O4) is produced by the reaction of salicylic acid (C7H6O3, Molar mass = 138.1 g/mol) and acetic anhydride (C4H6O3, Molar mass = 102.1 g/mol) based on the BALANCED equation : C7H6O3(s) + C4H6O3(l ) → C9H8O4(s) + C2H4O2( l) If 126.14 grams of aspirin (Molar mass = 180.2 g/mol) was collected from an experiment when 138.1 grams C7H6O3 reacted with excess C4H6O3, what was the percent yield?
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Combustion of hydrocarbons such as hexane (C6H₁4) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's 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. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid hexane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.220 kg of hexane are burned in air at a pressure of exactly 1 atm and a temperature of 17.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. ローロ X 0 x10