Combustion of urea CO{NH2)2)is described by the equation: The standard enthalpy

Question

Combustion of urea CO{NH2)2)is described by the equation: The standard enthalpy of combustion of urea is -632 kJ per mole of urea at 298 K. a) How much heat is either released or adsorbed per mole of oxygen consumed? b) The molar entropy of the combustion is 104.60 J K per mole of urea. Can you identify two distinct reasons why the combustion entropy is positive? What is the Gibbs free energy change of combustion per mole of urea at 298 K? Is it a spontaneous process? 10 pts c) Calculate the standard Gibbs energy of formation per mole of urea at 298K The - formation Gibbs free energy of CO2 = -394 kJ/mole and that of liquid water is -237 kJ/mole. 10 pts d) Does increasing the temperature stimulate combustion? Same question if the pressure is increased. 5 pts

Explanation / Answer

Answer - We are given,

The given combustion reaction

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---