(A) If the percent yield for the formation of urea in Example 4-13 were 87.5%, what mass...

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(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.

2 NH3(g) + CO(g) CO(NH2)2(s) + H,O(1)

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?


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General Chemistry Principles And Modern Applications

ISBN: 9780132931281

11th Edition

Authors: Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette

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