Question

What is ΔGo (in kJ) at 464 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)

Answer #1

**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)**

**delta H = delta Hf(PbCO3) - delta Hf(PbO) - delta
Hf(CO2)
= (-699.1) - (-219) - (-393.5)
= -86.6 KJ/mol
= -86600 J/mol**

**delta S = delta Sf(PbCO3) - delta Sf(PbO) - delta
Sf(CO2)
= (131) - (66.5) - (213.6)
= - 149.1 J/Kmol**

**Use:
delta G = delta H - T * delta S
= -86600 - (464)*(-149.1)
= -17417.6 J/mol
= -17.42 KJ/mol
Answer: -17.42 KJ/mol**

a) What is ΔGrxno (in kJ) at 2715 K for
the following reaction?
2POCl3(g) → 2PCl3(g) + O2(g)
POCl3(g): ΔHfo = -592.7 kJ/mol and
Sº = 324.6 J/K mol)
PCl3(g): ΔHfo = -287.0 kJ/mol and
Sº = 311.7 J/K mol)
O2(g): ΔHfo = ? kJ/mol and Sº =
205.0 J/K mol)
b) At what temperature (IN KELVIN) does the above reaction
become spontaneous?
c) What is ΔGrxno (in kJ) at 488 K for the
following reaction?
PbO(g) + CO2(g) →...

Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm
and 25 °C:
C2H6 (g) + O2 (g) →
CO2 (g) + H2O (l) (unbalanced)
ΔHf C2H6 (g) = -84.7 kJ/mol; S
C2H6 (g) = 229.5 J/K⋅mol;
ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S
CO2 (g) = 213.6 J/K⋅mol;
ΔHf H2O (l) = -285.8 kJ/mol; SH2O
(l) = 69.9 J/K⋅mol;
SO2 (g) = 205.0 J/K⋅mol

1. Given the values of ΔGfo given below in
kJ/mol, calculate the value of ΔGo in kJ for the
combustion of 1 mole of methane to form carbon dioxide and gaseous
water.
ΔGfo (CH4(g)) = -48
ΔGfo (CO2(g)) = -395
ΔGfo (H2O(g)) = -236
2.
Given the values of So given below in J/mol K and of
ΔHfo given in kJ/mol, calculate the value of
ΔGo in kJ for the combustion of 1 mole of ethane to form
carbon dioxide...

What is ΔGo (in kJ) at 79 ºC for the phase change of
nitromethane from the liquid to the gaseous state?
CH3NO2(l) → CH3NO2(g)
CH3NO2(l): ΔHfo = -113.1 kJ/mol and So = 171.8 J/K mol)
CH3NO2(g): ΔHfo = -74.7 kJ/mol and So = 274.4 J/K mol)

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) 180°C atm
(b) 460°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) 180°C atm
(b) 460°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) 100°C atm (b) 420°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

14.
What is ΔGo (in kJ) at 19 ºC for the phase change of
nitromethane from the liquid to the gaseous state?
CH3NO2(l) → CH3NO2(g)
CH3NO2(l): ΔHfo = -113.1 kJ/mol and So = 171.8 J/K mol)
CH3NO2(g): ΔHfo = -74.7 kJ/mol and So = 274.4 J/K mol)

13. 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) 160°C
____ atm
(b) 490°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

Calculate the enthalpy of reaction for the following reaction:
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔHfo(Fe2O3(s)) = -824.2 kJ/mol
ΔHfo(CO(g)) = -110.5 ΔHfo(Fe(s)) = ? ΔHfo(CO2(g)) = -393.5
kJ/mol

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