Answered: Nitric acid is a key industrial…

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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Question

Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that

899. liters per second of dioxygen are consumed when the reaction is run at 265.°C and the dioxygen is supplied at

0.23atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.

Expert Solution

Step 1

First we need to write a balanced chemical reaction for the ammonia and oxygen to produce nitrogen monoxide and water.

Using this reaction , we would write a relationship between rate of consumption of dioxygen and rate of production of nitrogen monoxide.

Then using the ideal gas equation we can calculate the moles of dioxygen consumed per second using the given volume , temperature and pressure.

From this we can calculate the rate of production of nitrogen monoxide in kg per second.

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