Determine the limiting reactant Express your answer as a chemical formula. Const

Question

Determine the limiting reactant Express your answer as a chemical formula. Constants I Periodic Table NH Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NHs) with carbon dioxide as follows 2 NHs (aq) +CO aq) CH&N;,0(aq)H2O(1) in an industrial synthesis of urea, a chemist combines 131.6 kg of ammonia with 211 4 kg of carbon dioxode and obtains 167 5 kg of urea Previous Answers Correct Part EB Determine the theoretical yield of urea Express your answer using four significant figures. m 2.144 kg Submit X Incorrect Try Again; 4 attempts remaining Part C Determine the percent yield for the reaction Express your answer using three significant figures.

Explanation / Answer

2NH3 + CO2------>CH4N2O +H2O

no of moles of NH3   = W/G.M.Wt

                                  = 131600/17   = 7741 moles

no of moles of CO2    = W/G.M.Wt

                                    = 211400/44    = 4804.5moles

1 moles of Co2 react with 2 moles of NH3

4804.5 moles of CO2 react with = 2*4804.5/1 = 9607 moles of NH3

NH3 is limiting reactant

2 moles of NH3 react with CO2 to gives 1 mole of CH4N2O

7741moles of NH3 react with Co2 to gives = 1*7741/2 = 3870.5 moles of CH4N2O

mass of urea   = no of moles * gram molar mass

                       = 3870.5*60 = 232230g of CH4N2O

The theoritical yield of urea   = 232230g   = 232.23Kg

percnt yield   =    actual yield/theoritical yield

                       = 167.5*100/232.23   = 72.13% >>>>>answer

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