(A) If the percent yield for the formation of urea in Example 4-13 were 87.5%, what mass of CO₂, together with an excess of NH₃ would have to be used to obtain 50.0 g CO(NH₂)₂?

(B) Calculate the mass of cyclohexanol (C₆H₁₁OH) needed to produce 45.0 g cyclohexene (C₆H₁₀) if the reaction has a 86.2% yield and the cyclohexanol is 92.3% pure.

Example 4-13

Billions of kilograms of urea, CO(NH₂)₂, are produced annually for use as a fertilizer.  A ball-and-stick model of urea is shown here. The reaction used is given  below.

The typical starting reaction mixture has a 3 : 1 mole ratio of NH₃ to CO₂ If  47.7 g urea forms per mole of CO₂ that reacts, what is the 

(a) Theoretical yield;  

(b) Actual yield; and 

(c) Percent yield?