We need to calculate the ΔGºf of CO(NH2)2 (s) using the following data: CO2(g) + 2NH3(g) --->...
We need to calculate the ΔGºf of CO(NH2)2 (s) using the following data:
CO2(g) + 2NH3(g) ---> H2O(g)
+ CO(NH2)2(s) .............ΔGº298=
1.91kJ
H2O(g) ---> 1/2O2(g) + H2(g)
....................................ΔGº298=
228.37kJ
C(graphite) + O2(g) ---> CO2(g)
...................................ΔGº298=-394.01kJ
N2(g) + 3H2(g) ---> 2NH3(g)
......................................ΔGº298=-33.24kJ
ΔGºf [CO(NH2)2(s)]= ?
How do we solve this? what is the process?
Homework Answers
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We need to calculate the ΔGºf of
CO(NH2)2 (s) using the following data:
CO2(g) + 2NH3(g) --->...
(ii) Calculate AH° for the reaction N2H4(1) + O2(g) → N2(g) + 2H2O(1) using the data...
(ii) Calculate AH° for the reaction N2H4(1) + O2(g) → N2(g) + 2H2O(1) using the data given below: 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(1) N2O(g) + 3H2(g) → N2H4(l) + H2O(1) 2NH3(g) + O2(g) → N2H4(1) + H2O(1) H2(g) + 1/2O2(g) → H2O(1) AH° = -1010. kJ AH° = -317 kJ AH° = -143 kJ AH° = -286 kJ
Consider the following reaction at 25 °C. CO2 (g) + 2NH3 (g) → CO(NH2 )2 (s)...
Consider the following reaction at 25 °C. CO2 (g) + 2NH3 (g) → CO(NH2 )2 (s) + H2 O(l) ; ∆H° = -134kJmol-1 Which of the following is correct regarding this reaction? (1) ∆S° is always a negative value for the reaction. (2) ∆H° increases with the temperature. (3) The decrease in the entropy change can determine the spontaneity of the reaction. (4) The reaction is spontaneous at all temperatures. (5) At high temperatures the value of ∆G° becomes more...
Given the following Thermodynamic data: CO2(g) H2O(l) NH3(g) CO(NH2)2(s) DeltaHof (kJ/mol): -393.5 -285.85 -45.9 -333.2 So...
Given the following Thermodynamic data: CO2(g) H2O(l) NH3(g) CO(NH2)2(s) DeltaHof (kJ/mol): -393.5 -285.85 -45.9 -333.2 So (J/K.mol): 214 70 193 105 (a) Calculate DeltaHo, DeltaSo, and DeltaGo at 25oC for the following reaction: CO2(g) + 2NH3(g) = CO(NH2)2(s) + H2O(l) (b) What is DeltaGo at 250oC? (Assume DeltaHo and DeltaSo do not change with temperature.) (c) Is the reaction spontaneous at each temperature? (Answer: (a) DeltaHo = -133.8 kJ; DeltaSo = -425 J/K; DeltaGo = -7.15 kJ; (b) DeltaGo =...
Given the following data for heats of reaction N2(g) + 3H2(g) ----> 2NH3(g) H = -91.8 kJ...
Given the following data for heats of reaction
N2(g) + 3H2(g) ---->
2NH3(g) H
= -91.8 kJ
C(graphite) + 2H2(g) ------->
CH4(g)H
= -74.9kJ
H2(g) + 2C(graphite) + N2(g)
--------> 2HCN(g) H
= 270.3 kJ
Calculate
H for the reaction used to make HCN
CH4(g) + NH3(g) --------> HCN(g) +
3H2(g)
Using the relevant S°values listed in Appendix G, calculate ΔS°298 for the following changes: (a) N2(g)+3H2(g)⟶2NH3(g)...
Using the relevant S°values listed in Appendix G, calculate ΔS°298 for the following changes: (a) N2(g)+3H2(g)⟶2NH3(g) (b) N2(g)+5/2O2(g)⟶N2O5(g)
Delta S is positive for the reaction ____. A) CaO (s) + CO2 (g)=>CaCO3 B) N2(g)...
Delta S is positive for the reaction ____. A) CaO (s) + CO2 (g)=>CaCO3 B) N2(g) + 3H2(g)=>2NH3(g) C) 2SO3(g) => 2SO2(g)+O2(g) D) Ag+(aq) + Cl- (aq)=> AgCl(s) E) H2) (l)=> H2O(s) I know that the answer is C, but I need a detailed explanation as to why the answer is C.
1:Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium...
1:Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0570 M, [H2] = 0.0420 M, [CO2] = 0.0860 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686°C. (b)If we add CO2 to increase its concentration to 0.440 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? (c) CO2: H2: CO: H2O: 2:The following...
Delta S is positive for the reaction__. a) CaO(s)+CO2(g)-->CaCO3(s) b) N2(g)+3H2(g)-->2NH3(g) c) 2SO3(g)--->2SO2(g) + O2(g) d)...
Delta S is positive for the reaction__. a) CaO(s)+CO2(g)-->CaCO3(s) b) N2(g)+3H2(g)-->2NH3(g) c) 2SO3(g)--->2SO2(g) + O2(g) d) Ag+(aq)+Cl-(aq)--->AgCl(s) e) H2O(l)--->H2O(s) *I know that C is the correct answer, I just need a detailed explanation as to why that is the correct answer.
Please explain Data: C(graphite) + O2(g) => CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) =>...
Please explain
Data: C(graphite) + O2(g) => CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) => H2O(1) AH = -285.8 kJ CH3OH(1) + 3/202(9) A CO2(g) + 2H20(1) AH = -726.4 kJ Using the data above, calculate the enthalpy change for the reaction below. Reaction: C(graphite) + 2H2(g) + 1/2O2(g) => CH3OH(1) A. +238.7 kJ B.-238.7 kJ C. +548.3 kJ D.-548.3 kJ E. +904.5 kJ
1. Using the relevant S'values listed in Appendix G, calculate AS 298 for the following changes...
1. Using the relevant S'values listed in Appendix G, calculate AS 298 for the following changes (a) N2(g)+3H2(g) +2NH3(g) (b) N2(g)+5/202(g)—N2O(g) 2. Use the standard free energy data in Appendix G to determine (1) AHan. (2) AS (3) AS., and Aune for cach of the following reactions, which are run under standard state conditions and 25 "C. Identify each as either spontaneous or nonspontaneous at these conditions. (a) C(s, graphite)+O2(g) CO2(g) (6) O2(g)+Nz/g/22NO(g) (c) Cu(s)+S(g)-Cu25(s) (d) CaO(s)+H20(1) Ca(OH)2(s) (e) Fe2O3(s)+3CO(g)...
(ii) Calculate AH° for the reaction N2H4(1) + O2(g) → N2(g) + 2H2O(1) using the data given below: 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(1) N2O(g) + 3H2(g) → N2H4(l) + H2O(1) 2NH3(g) + O2(g) → N2H4(1) + H2O(1) H2(g) + 1/2O2(g) → H2O(1) AH° = -1010. kJ AH° = -317 kJ AH° = -143 kJ AH° = -286 kJ
Given the following data for heats of reaction
N2(g) + 3H2(g) ---->
2NH3(g) H
= -91.8 kJ
C(graphite) + 2H2(g) ------->
CH4(g)H
= -74.9kJ
H2(g) + 2C(graphite) + N2(g)
--------> 2HCN(g) H
= 270.3 kJ
Calculate
H for the reaction used to make HCN
CH4(g) + NH3(g) --------> HCN(g) +
3H2(g)
Please explain
Data: C(graphite) + O2(g) => CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) => H2O(1) AH = -285.8 kJ CH3OH(1) + 3/202(9) A CO2(g) + 2H20(1) AH = -726.4 kJ Using the data above, calculate the enthalpy change for the reaction below. Reaction: C(graphite) + 2H2(g) + 1/2O2(g) => CH3OH(1) A. +238.7 kJ B.-238.7 kJ C. +548.3 kJ D.-548.3 kJ E. +904.5 kJ
1. Using the relevant S'values listed in Appendix G, calculate AS 298 for the following changes (a) N2(g)+3H2(g) +2NH3(g) (b) N2(g)+5/202(g)—N2O(g) 2. Use the standard free energy data in Appendix G to determine (1) AHan. (2) AS (3) AS., and Aune for cach of the following reactions, which are run under standard state conditions and 25 "C. Identify each as either spontaneous or nonspontaneous at these conditions. (a) C(s, graphite)+O2(g) CO2(g) (6) O2(g)+Nz/g/22NO(g) (c) Cu(s)+S(g)-Cu25(s) (d) CaO(s)+H20(1) Ca(OH)2(s) (e) Fe2O3(s)+3CO(g)...
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