Question

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^{-1}K^{-1}) |
||

ICl (l) | -23.89 | 135.1 | ||

ICl (g) | 17.78 | 247.6 |

Answer #1

**Answer** – Given, thermodynamic data of
∆H^{o}f anf S^{o}f and we need to calculated the
∆H^{o}f and ∆**S ^{o}**f for the
reaction as follow –

ICl(l) -----> ICl(g)

∆H^{o}f = Sum of the ∆H^{o}f product – sum of
the ∆H^{o}f of reactant

= 17.98 – (-23.89)

= 41.87 kJ/mol

∆S^{o}f = Sum of the S^{o}f product – sum of the
S^{o}f of reactant

= 247.6 – 135.1

= 112.5 J/mol

= 0.1125 kJ/mol. K

We know the formula

T = ∆H^{o}f / ∆S^{o}f

= 41.87 kJ.mol^{-1} / 0.1125
kJ.mol^{-1}.K^{-1}

= 372 K

the boiling point (in K) of ICl is **372 K**

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

Estimate ΔHrxn for the following chemical reaction
using the bond enthalpies in the table found here. 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!*

Estimate ΔHrxn for the following chemical reaction
using the bond enthalpies in the table found here. 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!*).
C2H2(g) + Cl2(g) →
C2H2Cl2(g)

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

Estimate ΔHrxn for the following chemical reaction
using the bond enthalpies in the table found here. 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!*).
C2H2(g) + Cl2(g) →
C2H2Cl2(g)
****** I WANT ANONYMOUS C WITH 1,300 ANSWERS TO ANSWER THIS
QUSTION !!!!!!!!!

Based on the thermodynamic properties provided for water,
determine the energy change when the temperature of 0.350 kg of
water decreased from 123 °C to 30.0 °C.
Property
Value
Units
Melting point
0
°C
Boiling point
100.0
°C
ΔHfus
6.01
kJ/mol
ΔHvap
40.67
kJ/mol
cp (s)
37.1
J/mol ·°C
cp (l)
75.3
J/mol ·°C
cp (g)
33.6
J/mol ·°C

Carbon disulfide (CS2) is a toxic, highly flammable substance.
The following thermodynamic data are available for CS2(l)
and CS2(g) at 298 K:
ΔH∘f (kJ/mol)
ΔG∘f (kJ/mol)
CS2(l)
89.7
65.3
CS2(g)
117.4
67.2
1. Liquid CS2 burns in O2 with a blue flame, forming
CO2(g) and SO2(g). Write a balanced equation for
this reaction.
2. Using the data in the preceding table and in Appendix C in
the textbook, calculate ΔH∘ and ΔG∘ for the
reaction in part D.
3. Use...

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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