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Problem: What is the percent yield for CH3Br if 12.23 g is produced when 5.00 g of CH4O reacts with excess HBr? CH4O + HBr → CH3Br + H2OA. 16% B. 67% C. 84% D. 82.6% E. 12%

FREE Expert Solution

We’re being asked to calculate the percent yield of CH3Br in the reaction of 5.00 g HBr with excess CH4O. The balanced chemical equation is:

 CH4O + HBr → CH3Br + H2O


Recall that percent yield is given by:


%yield = actual yieldtheoretical yieldx100



We know the reaction produced 12.23 g CH3Br; this is the actual yield of the reaction. To calculate the theoretical yield, we need to do the following:


Mass of CH4(molar mass of CH4O)  Moles of CH4(mole-to-mole comparison)  Moles of CH3Br (molar mass of CH3Br)  Mass of CH3Br


Since HBr is in excess, we can simply ignore it in our calculations.


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Problem Details

What is the percent yield for CH3Br if 12.23 g is produced when 5.00 g of CH4O reacts with excess HBr? CH4O + HBr → CH3Br + H2O

A. 16% 

B. 67% 

C. 84% 

D. 82.6% 

E. 12%

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