Reaction: CCl4 + HF → CCl2F2 + 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)
CCl4 + 2HF → CCl2F2 + 2HCl
C- 1 C - 1
Cl- 4 Cl -
1 2 F - 2
1 2 H - 1 2
Balanced equation: CCl4 + 2HF → CCl2F2 + 2HCl
Step 2: Moles CCl4
= 0.2139 mol CCl4
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.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Percent Yield concept. You can view video lessons to learn Percent Yield. Or if you need more Percent Yield practice, you can also practice Percent Yield practice problems.
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Based on our data, we think this problem is relevant for Professor Sonbuchner's class at Adelphi University.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.