Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction:
2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l)
Given that ΔG∘ = −13.6 kJ/mol, calculate ΔG at
25∘C for the following sets of conditions
Part A
50 atm NH3, 50 atm CO2, 4.0 M NH2CONH2
Express the free energy in kilojoules per mole to two
significant figures.
Part B
8.0×10−2 atm NH3, 8.0×10−2 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?
spontaneous for the conditions in both parts. |
nonspontaneous for the conditions in both parts. |
spontaneous for the conditions in Part but nonspontaneous for the conditions in Part B. |
spontaneous for the conditions in Part B but nonspontaneous for the conditions in Part A. |
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the following reaction: 2NH3(g)+CO2(g)→...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g)+CO2(g)→NH2CONH2(aq)+H2O(l) Given that ΔG∘ = -13.6 kJ, calculate ΔG at 25 ∘C for the following sets of conditions. (Figure 1) 1) 20 atm NH3, 20 atm CO2, 4.0 M NH2CONH2 2) 9.0×10−2 atm NH3, 9.0×10−2 atm CO2, 1.0 M NH2CONH2 Is the reaction spontaneous for the conditions in part (a) and/or part (b)? spontaneous for the conditions in part (b), nonspontaneous for the conditions in part (a) nonspontaneous...
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g)+CO2(g)?NH2CONH2(aq)+H2O(l) Given that ?G? = -13.6 kJ, calculate ?G at 25 ?C for the following sets of conditions. (Figure 1) Part A 40atm NH3, 40atm CO2, 3.0M NH2CONH2
Exercise 7.59 Part A Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows 2 NH3(aq) +CO2(aq)CH,N2O(a) H2() In an industrial synthesis of urea, a chemist combines 128.7 kg of ammonia with 211.4 kg of carbon dioxide and obtains 178.7 kg of urea Determine the limiting reactant Express your answer as a chemical formula Submit es ns Part B Determine the theoretical yield of urea Express your answer using...
The value of the equilibrium constant Kc for the reaction N2(g)+3H2(g)⇌2NH3(g) changes in the following manner as a function of temperature Temperature (∘C) Kc 300 9.6 400 0.50 500 0.058 Part A Use the standard enthalpies of formation given in Appendix C to determine the ΔH for this reaction at standard conditions. Express your answer in kilojoules to two decimal places. Part B If 0.027 mole of gaseous NH3 is added to a 1.00 L container and heated to 500 ∘C,...
Consider the following reaction: CO2(g)+CCl4(g)⇌2COCl2(g) Calculate ΔG for this reaction at25 ∘C under these conditions: PCO2PCCl4PCOCl2===0.115atm0.185atm0.750atm ΔG∘f for CO2(g) is −394.4kJ/mol, ΔG∘f for CCl4(g) is −62.3kJ/mol, and ΔG∘f for COCl2(g) is −204.9kJ/mol. Express the energy change in kilojoules per mole to one decimal place.
Consider the following reaction: CO2(g)+CCl4(g)⇌2COCl2(g) Calculate ΔG for this reaction at25 ∘C under these conditions: PCO2=0.100atm PCCl4=0.160atm PCOCl2=0.760atm ΔG∘f for CO2(g) is −394.4kJ/mol, ΔG∘f for CCl4(g) is −62.3kJ/mol, and ΔG∘f for COCl2(g) is −204.9kJ/mol. Express the energy change in kilojoules per mole to one decimal place.
Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Part A 315 K ΔG∘ Δ G ∘ = nothing kJ Part B 1085 K ΔG∘ Δ G ∘ = nothing kJ Part C 1465 K ΔG∘ Δ G ∘ = nothing kJ Part D Predict whether or not the reaction in part A will be spontaneous at 315...
2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 29 ∘C. Express your answer using four significant figures. Part A ΔG = ______ kJ Part B Is the reaction spontaneous? spontaneous OR nonspontaneous
Exercise 17.62 Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g). Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.) Part A 285 K ΔG∘ = 134 kJ SubmitMy AnswersGive Up Correct Part B 1095 K ΔG∘ = kJ SubmitMy AnswersGive Up Part C 1475 K ΔG∘ = −50.9 kJ SubmitMy AnswersGive Up Incorrect; Try Again; 5 attempts remaining Part D Predict whether or not the reaction...
1. The simplest ammonia formation is from nitrogen and hydrogen. Consider the reversible reaction N2(g) + 3H2(g) → 2NH3(g) The standard enthaply and Gibbs free energy of formation one mole NH3 is ∆H◦ m = −46.11 kJ mol−1 and ∆G◦ m = −16.78 kJ mol−1 . (a) What is equilibrium constant at standard condition (25°C and 1 atm)? (b) What is equilibrium constant at 60°C and 1 atm? (c) What is the Gibbs free-energy change relative to that under standard...