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

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!*

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)

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

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 !!!!!!!!!

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...

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...

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