part A Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrial

Question

part A Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction: 2NH3(g)+CO2(g)NH2CONH2(aq)+H2O(l) Given that G = 13.6 kJ/mol, calculate G at 25C for the following sets of conditions. (Figure 140 atm NH3, 40 atm CO2, 5.0 M NH2CONH2 Express the free energy in kilojoules per mole to two significant figures. Part B 5.0×102 atm NH3, 5.0×102 atm CO2, 1.0 M NH2CONH2 Express the free energy in kilojoules per mole to two significant figures. Part C Is the reaction spontaneous for the conditions in Part A and/or Part B? The reaction is Is the reaction spontaneous for the conditions in Part A and/or Part B? nonspontaneous for the conditions in both parts. spontaneous for the conditions in Part A but nonspontaneous for the conditions in Part B. spontaneous for the conditions in Part B but nonspontaneous for the conditions in Part A. spontaneous for the conditions in both parts.

Explanation / Answer

The reaction is 2NH3+CO2-----àNH2CO.NH2+H2O

deltaG= deltaGo+RT*lnQ

Q= [NH2CONH2/ (PCO2*PNH32)

P indicates parital pressure

. (Figure 140 atm NH3, 40 atm CO2, 5.0 M NH2CONH2

Part A ; Q=5/(40*140*140)= 6.377*10-6

deltaG = -13.6*1000 (J/mole)+8.314*298*ln(6.377*10-6)= -43238.5 Kj/mole. Since delta G is –ve the reaction is spontaneous.

Part B 5.0×102 atm NH3, 5.0×102 atm CO2, 1.0 M NH2CONH2

Part B : Q= 1/(5*10-2*5*10-2*5*10-2)= 8000

deltaG = -13.6*1000+8.314*298*ln(8000)= 8666.4, since deltaG is +ve, the reaction is snot spontaneous.

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