Inorganic Geochemisrty…………. RE: Thermodynamics….,.. Given: ΔHf° (J) Sf°(J/mole*k) Quartz -217650 9.88 Grossular -1582737 60.87 Anorthite -1007552...
Inorganic Geochemisrty…………. RE: Thermodynamics….,..
Given:
ΔHf° (J) Sf°(J/mole*k)
Quartz -217650 9.88
Grossular -1582737 60.87
Anorthite -1007552 49.1
Wollastonite -389590 19.60
1. Solve Gibbs Free Energy change.
2. Calculate Entropy formation for qtz, Gross, Anorth, Wollas …..
3. At standard state conditios, is it endothermic or esothermic…..
4. Which is stable at standard state conditions.
Homework Answers
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Inorganic Geochemisrty…………. RE:
Thermodynamics….,..
Given:
ΔHf° (J) Sf°(J/mole*k)
Quartz -217650 9.88
Grossular -1582737 60.87
Anorthite -1007552...
kJ/mole) The standard enthalpy of combustion of solid urea (NH2 (C-O) (C=O)NH2 ) is -632 kJ/mole...
kJ/mole) The standard enthalpy of combustion of solid urea (NH2 (C-O) (C=O)NH2 ) is -632 kJ/mole under standard conditions. Its standard molar entropy is 104.60 J/K mol. Calculate the Gibbs energy of formation of urea at 298K.(ANS: -663 kJ/mol) 4.
What is the change in volume for this reaction (ΔVR(1 bar, 298K)) at 298K and 1...
What is the change in volume for this reaction (ΔVR(1 bar,
298K)) at 298K and 1 bar? Are the products or reactants denser?
What is the change in enthalpy for this reaction (ΔHR(1 bar,
298K)) at 298K and 1 bar? Is the reaction exothermic or
endothermic?
What is the change in internal energy for this reaction (ΔER(1
bar, 298K)) at 298K and 1 bar? For this reaction, under these
conditions is q or w the more significant term?
What is...
JOY 20 $49.4 J/mol K -899.0 /mol K 7. According to the second law of thermodynamics,...
JOY 20 $49.4 J/mol K -899.0 /mol K 7. According to the second law of thermodynamics, the change in the entropy of the universe (DS...) during a spontaneous reaction is a ero b negative positive. d less than the change in entropy of the system (DS.). greater than the change in entropy of the system (DS). 8. In an experiment, 1.000 mol of sodium metal is placed in a container and reacted with 4.000 mol of chlorine given the following....
4. (a) Calculate the Gibbs Free Energy of formation for urea at 25°C. Given: The standard...
4. (a) Calculate the Gibbs Free Energy of formation for urea at 25°C. Given: The standard enthalpy of formation is -333.17 kJ mol and the standard entropy of formation is 136.093 J K mol". (b) is the formation of urea a spontaneous process under these conditions? Explain. (7 pts) J mol
Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the...
Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the reaction of dissolving silver sulfide, Ag2S, in water (25 C.) Do the calculations in two ways. Use the standard Enthalpy of formation, deltaH, and entropy S values, and the formula deltaG=deltaH-TdeltaS. Use the standard free energies of formation deltaG and the formula deltaG=deltaG(products)-deltaG(reactants).
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7...
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.
Chapter 1 Thermodynamics Page 16 16. The standard enthalpy of combustion of solid phenol (CH3OH) is...
Chapter 1 Thermodynamics Page 16 16. The standard enthalpy of combustion of solid phenol (CH3OH) is -3054 kJ moli' at 298K and its standard molar entropy is 144,0 J K'moll. Calculate the standard Gibbs free energy of formation at 298K. (81,98 kJ mol) 17. Calculate the standard Helmholtz energy of formation of CH2OH(l) at 298K from the standard Gibbs energy of formation, on the assumption that He and O2 are perfect gases. (-160 kJ mol') 18. a. Calculate the heat...
Need help on this thermodynamics question. Thanks Data given from function Cp=22.64 + 6.28 x (10^-3)*T...
Need help on this thermodynamics question. Thanks
Data given from function Cp=22.64 + 6.28 x (10^-3)*T [Jmol-1 K-1
]
Cp(J/mol.K) T(K) 24.524 300 24.838 350 400 25.152 25.466 450 500 25.78 550 26.408 26.722 650 27.036 700 750 27.35 27.664 800 27.978 28.292 28.606 950 1000 28.92 1050 29.234 1100 29.548 1150 29.862 30.176 1200 1250 30.49 1300 30.804 1350 31.118 358 31.16824 The specific heat capacity of solid copper above 300 K is given by Cp-22.64+6.28 x 103TJmol K1]...
23 p 30+ ody 1 Determines le for the reason 30.09) given the following information Slemelk)...
23 p 30+ ody 1 Determines le for the reason 30.09) given the following information Slemelk) 4 F Substance Fe O.) Feca) 0.6) 273 205.0 a -144.9 J/mol K d -549.4 mol K 549.4 J/mol K +1449/mol 899.0 /mol K 7. According to the second law of thermodynamics, the change in the entropy of the universe (DS...) during spontaneous reaction is b negative c. positive d less than the change in entropy of the system (DS...) e greater than the...
21.) Consider the standard free energies shown below(T =37 °C, R-8.3 145 J/mole K) : UDP-Glucuronate...
21.) Consider the standard free energies shown below(T =37 °C, R-8.3 145 J/mole K) : UDP-Glucuronate + H20 UTP+ H2O M+ Pi+ PPE+ H202Pi AG =-36.9 kJ/mol 39 AG =-32.5 kJ/mol -32.5 AG-33.6 kJ/mol 1-Phosphoglucuronate+UMP+ (A) (3 pts) Calcul ate AG & Keg for the following reaction. 1-Phosphoglucuronate + UTP + H2O UDP-Glucuronate + 2Pi (B) (2 pts) Which of the following statements best describe this reaction? (A)The reaction is irreversible under standard conditions. (B) The reaction is reversible under...
kJ/mole) The standard enthalpy of combustion of solid urea (NH2 (C-O) (C=O)NH2 ) is -632 kJ/mole under standard conditions. Its standard molar entropy is 104.60 J/K mol. Calculate the Gibbs energy of formation of urea at 298K.(ANS: -663 kJ/mol) 4.
What is the change in volume for this reaction (ΔVR(1 bar,
298K)) at 298K and 1 bar? Are the products or reactants denser?
What is the change in enthalpy for this reaction (ΔHR(1 bar,
298K)) at 298K and 1 bar? Is the reaction exothermic or
endothermic?
What is the change in internal energy for this reaction (ΔER(1
bar, 298K)) at 298K and 1 bar? For this reaction, under these
conditions is q or w the more significant term?
What is...
JOY 20 $49.4 J/mol K -899.0 /mol K 7. According to the second law of thermodynamics, the change in the entropy of the universe (DS...) during a spontaneous reaction is a ero b negative positive. d less than the change in entropy of the system (DS.). greater than the change in entropy of the system (DS). 8. In an experiment, 1.000 mol of sodium metal is placed in a container and reacted with 4.000 mol of chlorine given the following....
4. (a) Calculate the Gibbs Free Energy of formation for urea at 25°C. Given: The standard enthalpy of formation is -333.17 kJ mol and the standard entropy of formation is 136.093 J K mol". (b) is the formation of urea a spontaneous process under these conditions? Explain. (7 pts) J mol
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.
Chapter 1 Thermodynamics Page 16 16. The standard enthalpy of combustion of solid phenol (CH3OH) is -3054 kJ moli' at 298K and its standard molar entropy is 144,0 J K'moll. Calculate the standard Gibbs free energy of formation at 298K. (81,98 kJ mol) 17. Calculate the standard Helmholtz energy of formation of CH2OH(l) at 298K from the standard Gibbs energy of formation, on the assumption that He and O2 are perfect gases. (-160 kJ mol') 18. a. Calculate the heat...
Need help on this thermodynamics question. Thanks
Data given from function Cp=22.64 + 6.28 x (10^-3)*T [Jmol-1 K-1
]
Cp(J/mol.K) T(K) 24.524 300 24.838 350 400 25.152 25.466 450 500 25.78 550 26.408 26.722 650 27.036 700 750 27.35 27.664 800 27.978 28.292 28.606 950 1000 28.92 1050 29.234 1100 29.548 1150 29.862 30.176 1200 1250 30.49 1300 30.804 1350 31.118 358 31.16824 The specific heat capacity of solid copper above 300 K is given by Cp-22.64+6.28 x 103TJmol K1]...
23 p 30+ ody 1 Determines le for the reason 30.09) given the following information Slemelk) 4 F Substance Fe O.) Feca) 0.6) 273 205.0 a -144.9 J/mol K d -549.4 mol K 549.4 J/mol K +1449/mol 899.0 /mol K 7. According to the second law of thermodynamics, the change in the entropy of the universe (DS...) during spontaneous reaction is b negative c. positive d less than the change in entropy of the system (DS...) e greater than the...
21.) Consider the standard free energies shown below(T =37 °C, R-8.3 145 J/mole K) : UDP-Glucuronate + H20 UTP+ H2O M+ Pi+ PPE+ H202Pi AG =-36.9 kJ/mol 39 AG =-32.5 kJ/mol -32.5 AG-33.6 kJ/mol 1-Phosphoglucuronate+UMP+ (A) (3 pts) Calcul ate AG & Keg for the following reaction. 1-Phosphoglucuronate + UTP + H2O UDP-Glucuronate + 2Pi (B) (2 pts) Which of the following statements best describe this reaction? (A)The reaction is irreversible under standard conditions. (B) The reaction is reversible under...
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