Question

Using the thermodynamic data provided below, calculate Ksp for ZnS(s) at 25°.

Calculate Ksp for ZnS(s) | 'H°f (kJ/mol) | S° (J/K·mol) |

Zn^2+(aq) | -152.4 | -106.5 |

S^2–(aq) | 41.8 | 22 |

ZnS (s) | -203 | 57.7 |

Answer #1

The thermodynamic properties for the species involved in the
Zn(s)|Zn2+(aq)||Pb2+(aq)|Pb(s) cell are given
below.
Substance
∆G°f
kJ/mol
S°
J/K*mol
∆H°f
kJ/mol
Zn(s)
0
41.63
0
Pb(s)
0
64.81
0
Zn2+(aq)
-147.06
-112.1
-153.89
Pb2+(aq)
-24.43
10.5
-1.7
Calculate ∆G°, ∆S° and
∆H° for the chemical reaction
occuring in the cell.Is the reaction spontaneous? Is this a
favorable entropy change? Favorable energy change?

Use the thermodynamic data provided below to determine ΔG (in
kJ/mol) for the condensation of C2H5OH at
64.02 °C if the initial partial pressure of
C2H5OH is 1.99 atm. Report your answer to one
decimal place in standard notation (i.e. 123.4 kJ/mol).
Substance
ΔH°f (kJ/mol)
S° (J mol-1K-1)
C2H5OH (l)
-277.7
160.7
C2H5OH (g)
-235.1
282.7

Use the thermodynamic data provided below to determine ΔG (in
kJ/mol) for the vaporization of CaO at 91.8 °C if the initial
partial pressure of CaO is 1.76 atm. Report your answer to one
decimal place in standard notation (i.e. 123.4 kJ/mol).
Substance
ΔH°f (kJ/mol)
S° (J mol-1K-1)
CaO (l)
-557.3
62.3
CaO (g)
43.9
219.7

Use the thermodynamic data provided below to determine ΔG (in
kJ/mol) for the condensation of NaCl at 138.08 °C if the initial
partial pressure of NaCl is 1.62 atm. Report your answer to one
decimal place in standard notation (i.e. 123.4 kJ/mol).
Substance
ΔH°f (kJ/mol)
S° (J mol-1K-1)
NaCl (l)
-385.9
95.1
NaCl (g)
-181.4
229.8

Use the thermodynamic data provided below to estimate the
boiling point (in K) of ICl. Report your answer to zero decimal
places in standard notation (i.e. 123. kJ *For numbers ending in
zero, be sure to include the decimal!*).
Substance
ΔH°f (kJ/mol)
S° (J mol-1K-1)
ICl (l)
-23.89
135.1
ICl (g)
17.78
247.6

Using a Table of thermodynamic data, calculate the change in
Gibbs free energy for each of the following reactions. In each case
indicate whether the reaction is spontaneous under standard
conditions. Here are some more delta G values: N2H4 (g) = 159.4
kJ/mol, FeO (s) = -255.2 kJ/mol, FeCl3 (s) = -334 kJ/mol, H3PO4
(aq) = -1142.6 kJ/mol
(a) 2 Fe(s) + O2(g)--->2 FeO(s) kJ
(b) 2 SO2(g) + O2(g)--->2 SO3(g) kJ
(c) 4 Al(s) + 3 O2(g)--->2Al2O3(s) kJ
(d)...

Use the thermodynamic data below to determine the equilibrium
constant for the conversion of oxygen to ozone at 3803°C
3O2 (g) ⇌ 2O3
(g)
substance ΔH˚f
(kJ/mol) ΔG˚f
(kJ/mol) S˚ (J/mol*K)
O2
(g) 0 0 205.0
O3
(g) 142.3
163.4
237.6

Using a thermodynamic table below , determine the bond energy of
F2, along with the fraction of diatomics that have sufficient
energy to react at 298K and 500K.
ΔH°f (kJ mol-1)
ΔG°f (kJ mol-1)
S°m (J mol-1 K-1)
Cp,m (J mol-1 K-1)
Molecular weight
F2(g)
0
0
202.8
31.3
38.00
F(g)
79.4
62.3
158.8
22.7
19.00

Using values from the Appendix of Thermodynamic data, calculate
the value of H° for each of the following reactions.
(a) Fe2O3(s) + 6 HCl(g) 2 FeCl3(s) + 3 H2O(g) H° = kJ
(b) 2 H2S(g) + 3 O2 (g) 2 SO2 (g) + 2 H2O(g) H° = kJ
(c) NaOH(s) + CO2(g) NaHCO3(s) H° = kJ
(d) 4 NH3(g) + O2(g) 2 N2H4(g) + 2 H2O(l) H° = kJ

1)Use standard thermodynamic data (in the Chemistry References)
to calculate G at 298.15 K for the following reaction, assuming
that all gases have a pressure of 19.31 mm Hg. 2N2(g) +
O2(g)2N2O(g)
G = ? kJ/mol
2)Using standard thermodynamic data (linked), calculate the
equilibrium constant at 298.15 K for the following reaction.
C2H4(g) + H2O(g)CH3CH2OH(g)
K = ?
3) Calculate the temperature (in kelvins) at which the sign of
G° changes from positive to negative for the reaction below. This...

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