1-What is ΔGrxno (in kJ) at 338 K for the
following reaction?
PbO(g) + CO2(g) → PbCO3(s)
PbO: ΔHfo = -219.0 kJ/mol and So =
66.5 J/K mol)
PbCO3(s): ΔHfo = -699.1 kJ/mol and
So = 131.0 J/K mol)
CO2: ΔHfo = -393.5 kJ/mol and
So = 213.6 J/K mol)
2-At what temperature (in K) does the above reaction become spontaneous?
PLEASE answer both
1-What is ΔGrxno (in kJ) at 338 K for the following reaction? PbO(g) + CO2(g) →...
What is ΔGo (in kJ) at 647 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) At what temperature (in K) does the above reaction become spontaneous?
1.What is ΔGrxno (in kJ) at 440 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) 2. At what temperature (in K) does the above reaction become spontaneous?
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for : Mark 1.00 out of 1.00 2002(g) +4H2O(1) ► 2CH3OH(1) + 302(g) P Flag question Answer: 1404.84 Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AGⓇ =AH°-TAS and assume AH° and AS are independent of temperature. P Flag question (Theis...
(2 pts) Calculate the equilibrium pressure of CO2 in the system at 3000C. ΔH0 = 88.3 kJ and ΔS0 = 151.3 J/K. R = 8.314 J/mol K PbCO3(s) ® PbO(s) + CO2(g) ΔH0f(kJ/mol) -699.1 -217.3 -393.5 S0(J/mol K) 131 68.7 213.6
Consider the reaction shown below. PbCO3(s) PbO(s) + CO2(g) Calculate the equilibrium pressure of CO2 in the system at the following temperatures. (a) 300°C ____atm (b) 550°C _____atm Note: To find the value of the equilibrium constant at each temperature you must first find the value of G0 at each temperature by using the equation G0 = H0 - TS0 For this reaction the values are H0 = +88.3 kJ/mol and S0= 151.3 J/mol*K
Consider the reaction shown below. PbCO3(s) PbO(s) + CO2(g) Calculate the equilibrium pressure of CO2 in the system at the following temperatures. (a) 240°C ? atm (b) 600°C ? atm Note: To find the value of the equilibrium constant at each temperature you must first find the value of G0 at each temperature by using the equation G0 = H0 - TS0 For this reaction the values are H0 = +88.3 kJ/mol and S0= 151.3 J/mol*K
need it asap plz 1) Consider the following reaction: CO(g) + H2O(g) + H2(g) + CO2(B) AHP (l/mol) -110.5 -241.8 -393.5 SU/K-mol) 197.9 188.7 131.0 213.6 a. Calculate the Standard Gibbs Free Energy (AG) and determine whether the reaction is spontaneous in the forward direction at 374K. (374K was chosen because it's just above the normal boiling point of water, which is the lowest temperature where the "standard" 1atm of water vapor can exist.) b. Calculate the equilibrium constant for...
Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AG° =AH° -TAS® and assume AH° and 4Sº are independent of temperature. P Flag question (Theº is included because it is still for standard conditions, that is, 1 atm for gases and 1 molar for concentrations.) Answer: What is Agrº (in kJ) at 2268 K for the following...
What temperature must the reaction be above in order to become spontaneous? CaCO3(s)CaO(s)+CO2(9) AHor (CaCO3)-1207.6 k]/mol So (CaCO3) 91.7 J/mol K AHof (CaO)-35.09 kJ/mol S° (CaO) 38.2 J/mol K AHor (CO2)-393.51 kJ/mol So (CO2)213.74 J/mol K