**Polyacrylonitrile Production Analysis**Polyacrylonitrile is a polymer widely used in the production of bicycle frames, tennis rackets, and airplane frames. It is manufactured from the monomer acrylonitrile, which is produced in large quantities in the chemical industry.**Reaction Overview**Using the balanced equation below for the synthesis of acrylonitrile, determine the amount of acrylonitrile that can be produced under given conditions and calculate the percent yield for this reaction:\[ 2\text{C}_3\text{H}_6(\text{g}) + 2\text{NH}_3(\text{g}) + 3\text{O}_2(\text{g}) \rightarrow 2\text{C}_3\text{H}_3\text{N}(\text{g}) + 6\text{H}_2\text{O}(\text{g}) \]**Experimental Setup**A local chemical company produces a batch of acrylonitrile using the following reactants:- 1.00 kg of propylene (C\(_3\)H\(_6\), MW 42.08 g/mol)- 1.50 kg of ammonia (NH\(_3\), MW 17.03 g/mol)- 2.00 kg of oxygen (O\(_2\), MW 32.00 g/mol)Set up the table below to represent a 100% yield under the specified reaction conditions. Ignore the water side product.**Reaction Table**| Component | 2C\(_3\)H\(_6\)(g) | 2NH\(_3\)(g) | 3O\(_2\)(g) | 2C\(_3\)H\(_3\)N(g) ||--------------|-------------|----------|----------|------------|| Before (mol) | | | | || Change (mol) | | | | || After (mol) | | | | |**Instructions**- Calculate the number of moles for each reactant before the reaction.- Determine the change in moles as the reaction progresses.- Calculate the number of moles remaining after the reaction.Adjust the values appropriately in the table to show a complete reaction with 100% yield, focusing only on

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Using the balanced equation for the synthesis of acrylonitrile (below), determine the amount of acrylonitrile that can be produced under the following conditions and the percent yield for this reaction. 2C3H6(g) + 2NH3(g) + 302(g) → 2C;H;N(g) + 6H20(g) 4. NEXT > The local chemical company makes a batch of acrylonitrile using 1.00 kg of propylene (C3H6, MW 42.08 g/mol), 1.50 kg of ammonia (NH, MW 17.03 g/mol) and 2.00 kg of oxygen (O2, MW 32.00 g/mol). Set up the table below that represents 100% yield with the given reaction conditions. Ignore the water side product. 2C3H6(g) 2NH3(g) 302(g) 2C,H;N(g) Before (mol) Change (mol) After (mol)

Using the balanced equation for the synthesis of acrylonitrile (below), determine the amount of acrylonitrile that can be produced under the following conditions and the percent yield for this reaction. 2C3H6(g) + 2NH3(g) + 302(g) → 2C;H;N(g) + 6H20(g) 4. NEXT > The local chemical company makes a batch of acrylonitrile using 1.00 kg of propylene (C3H6, MW 42.08 g/mol), 1.50 kg of ammonia (NH, MW 17.03 g/mol) and 2.00 kg of oxygen (O2, MW 32.00 g/mol). Set up the table below that represents 100% yield with the given reaction conditions. Ignore the water side product. 2C3H6(g) 2NH3(g) 302(g) 2C,H;N(g) Before (mol) Change (mol) After (mol)

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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