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Problem: Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of CCl4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.

🤓 Based on our data, we think this question is relevant for Professor Sonbuchner's class at Adelphi University.

FREE Expert Solution

ReactionCCl4 + HF  CCl2F+ HCl 


For this problem we need to do these steps:


Step 1: Write the balanced equation for the reaction 

Step 2: Determine moles CCl4 reacted using its molar mass and its given mass 

Step 3: Calculate the theoretical yield (in g) of CCl2F2 stoichiometrically (mole to mole comparison) and its molar mass (mole to mass calculation)

Step 4: Calculate percent yield using the actual yield and theoretical yield 


Step 1: Balanced equation (add coefficients)


CCl42HF  CCl2F2HCl 

reactants               products

C- 1                   C - 1

Cl- 4                  Cl - 3 4  

F- 1 2                 F - 2

H- 1 2                 H - 1 2  


Balanced equation: CCl42HF  CCl2F2HCl 


Step 2: Moles CCl4

  • Molar mass CCl4 = 153.82 g/mol


32.9 g CCl4×1 mol CCl4153.82 g CCl40.2139 mol CCl4

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Problem Details

Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of CCl4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.