Chemistry for Engineering Students
Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Textbook Question
Chapter 4, Problem 4.72PAE

4.80 The reaction shown below is used to destroy Freon-12 (CF2Cl2), preventing its release into the atmosphere. What mass of NaF will be formed if 250.0 kg of CF2Cl2 and 400.0 kg of Na2C2O4 are heated and allowed to react to completion?

   CF 2 Cl 2 +  2 Na 2 C 2 O 4    2 NaF  +  2 NaCl  +  C  +  4CO 2

Expert Solution & Answer
Check Mark
Interpretation Introduction

Interpretation:

To calculate the mass of sodium fluoride required for the process.

Concept introduction:

  • Use the stoichiometric ratios in order to verify the total amount of moles
  • Use molar masses to calculate mass and moles.

Answer to Problem 4.72PAE

Solution:

125.31 kg

Given:

 m = 250.0 kg of CF2Cl2 m = 400.0 kg of Na2C2O4

Explanation of Solution

Use stoichiometry to relate the amounts of moles of CF2Cl2 and phosphoric acid. Then use molar masses to calculate the mass of each material.

Verify the limiting reactant, and base the final calculation of sodium fluoride with the given species.

1st step. Calculate moles of each species

mol CF2Cl2 = mass molarmass =  ( 250.0 kg ) 120.91 kg/kmol = 2.067 kmolmol Na2C2O4 =  mass molarmass=  ( 400.0.0 kg ) 134.0 kg/kmol = 2.985 kmol

2nd step. Verify ratio of species

 2 mol of Na2C2O4 = 1 mol of CF2Cl2         2.985 kmol of Na2C2O4 = 1.4925 kmol of CF2Cl2Clearly, Na2C2O4 is limiting the reaction, CF2Cl2 is in excess

 

3rd step: Calculate moles of NaF required .

2 mol of Na2C2O4 =2 mol of NaF 2.985 kmol of Na2C2O4 = 2.985 kmol of NaF

4th step: Calculate mass of NaF

Mass = mol x (MolarMass) Mass = (2.985 kmol of NaF)x( 41.98 g/mol)Mass= 125.31 kg

Conclusion

The total mass of NaF produced to for this process is 125.31 kg

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Chapter 4 Solutions

Chemistry for Engineering Students

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