Question
In: Chemistry
Use ?G?f values from Appendix IIB to calculate the equilibrium constants at 25 ?C for each...
Use ?G?f values from Appendix IIB to calculate the equilibrium constants at 25 ?C for each of the following reactions.
a. 2NO2(g)?N2O4(g)
b. 3/2H2(g)+1/4P4(g)?PH3(g)
Solutions
Expert Solution
a. 2NO2(g)---------------------> N2O4(g)
Grxn
=
Gproducts -
Greactants
= 99.8 - (2 x 51.3)
= -2.8 kJ / mol
Grxn
= - R T ln K
-2.8 = -(8.314 x 10^-3 ) x 298 x ln K
ln K = 1.13
K = 3.10
equilibrium constant = K = 3.10
b. 3/2H2(g)+1/4P4(g)-----------------> PH3(g)
Grxn
=
Gproducts -
Greactants
= 13.5 - (1/4 x 24.4)
= 7.4 kJ / mol
Grxn
= - R T ln K
7.4 = -(8.314 x 10^-3 ) x 298 x ln K
ln K = -2.99
K = 0.050
equilibrium constant = K = 0.050
queen_honey_blossom answered 1 year agoRelated Solutions
Use data from Appendix IIB in the textbook to calculate the equilibrium constants at 25?C for...
Use data from Appendix IIB in the textbook to calculate the
equilibrium constants at 25?C for each of the following
reactions.
2NO(g)+O2(g)?2NO2(g) .
Express your answer using two significant figures.
Use data from the table below to calculate the equilibrium constants at 25 ∘C for each...
Use data from the table below to calculate the equilibrium
constants at 25 ∘C for each reaction.
Standard Thermodynamic Quantities for Selected Substances
at 25∘C
Substance
ΔH∘f(kJ/mol)
ΔG∘f(kJ/mol)
S∘(J/mol⋅K)
H2(g)
0
0
130.7
N2(g)
0
0
191.6
Br2(g)
30.9
3.1
245.5
Cl2(g)
0
0
223.1
NO2(g)
33.2
51.3
240.1
N2O4(g)
9.16
99.8
304.4
NH3(g)
-45.9
-16.4
192.8
P4(g)
58.9
24.4
280.0
PH3(g)
5.4
13.5
210.2
Part A
2NO2(g)⇌N2O4(g)
Find K
Part B
Br2(g)+Cl2(g)⇌2BrCl(g)
ΔG∘f for BrCl(g) is -1.0 kJ/mol
Find...
Use data from Appendix C to calculate the equilibrium constant, K, and ΔG∘ at 298 K...
Use data from Appendix C to calculate the equilibrium constant,
K, and ΔG∘ at 298 K for each of the following
reactions.
H2(g)+I2(g)⇌2HI(g)
Calculate ΔG∘.
Express your answer to four significant figures and include the
appropriate units.
Part A
H2(g)+I2(g)⇌2HI(g)
Calculate ΔG∘.
Express your answer to four significant figures and include the
appropriate units.
Part B
Calculate the equilibrium constant, K.
Express your answer using two significant figures.
Part C
C2H5OH(g)⇌C2H4(g)+H2O(g)
Calculate ΔG∘.
Express your answer to two significant figures...
Using S? values from Appendix C in the textbook, calculate ?S? values for the following reactions....
Using S? values from Appendix C in the textbook, calculate ?S?
values for the following reactions. 5 significant figures
please!!!
C2H4(g)+H2(g)?C2H6(g)
N2O4(g)?2NO2(g)
Be(OH)2(s)?BeO(s)+H2O(g)
2CH3OH(g)+3O2(g)?2CO2(g)+4H2O(g)
Using values from the Appendix of Thermodynamic data, calculate the value of H° for each of...
Using values from the Appendix of Thermodynamic data, calculate
the value of H° for each of the following reactions.
(a) 3 Fe(s) + 4 CO2(g) 4 CO(g) + Fe3O4(s)
H° = 13.6
Correct: Your answer is correct.
kJ
(b) CH4(g) + 4 Cl2(g) CCl4(l) + 4 HCl(g)
H° = 308.6
Incorrect: Your answer is incorrect.
kJ
(c) Fe2O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(g)
H° = 24.8
Incorrect: Your answer is incorrect.
kJ
(d) 4 NH3(g) + O2(g)...
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...
Calculate the equilibrium constant for each of the reactions at
25∘C.
Standard Electrode Potentials at 25 ∘C
Reduction Half-Reaction
E∘(V)
Fe3+(aq)+3e−
→Fe(s)
-0.036
Sn2+(aq)+2e−
→Sn(s)
-0.14
Ni2+(aq)+2e−
→Ni(s)
-0.23
O2(g)+2H2O(l)+4e−
→4OH−(aq)
0.40
Br2(l)+2e−
→2Br−
1.09
I2(s)+2e−
→2I−
0.54
Part A
2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq)
Express your answer using two significant figures.
Part B
O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq)
Express your answer using two significant figures.
Part C
Br2(l)+2I−(aq)→2Br−(aq)+I2(s)
Express your answer using two significant figures.
Using values from Appendix C of your textbook, calculate the value of Ho, So, and Go...
Using values from Appendix C of your textbook, calculate the
value of Ho, So, and Go for each of the following reactions at
standard temperature (298 K). Next calculate G if ALL of the GASSES
in the reaction have partial pressures of 0.2 atm.
(a) NaOH(s) + CO2(g) NaHCO3(s) Ho = -127.44 kJ/mol
So = -176.02 J/mol-K
Go = -74.96 kJ/mol
If all gasses have partial pressures of 0.2 atm then G =
________ kJ/mol.
(b) 2 Fe(s) + 3...
Equilibrium constants at 25 ?C are listed in the table below. Substance Kc Value of Kc...
Equilibrium constants at 25 ?C
are listed in the table below.
Substance
Kc
Value of Kc
CaCO3
Ksp
4.5
Equilibrium constants at 25 ?C are listed in the table below. Substance Kc Value of Kc...
Equilibrium constants at 25 ?C are listed in the table
below.
Substance
Kc
Value of Kc
CaCO3
Ksp
4.5�10?9
H2CO3
Ka1
4.3�10?7
Ka2
5.6�10?11
What is the molar solubility of marble (i.e., [Ca2+] in a
saturated solution) in normal rainwater, for which pH=5.60?
Express your answer to two significant figures and include the
appropriate units.
From the following equilibrium constants, calculate the equilibrium constant for the reaction HO2CCO2H ----->2H+ + C2O-24...
From the following equilibrium constants, calculate the
equilibrium constant for the reaction
HO2CCO2H ----->2H+ +
C2O-24
k1=5.6x10-2
k2=5.4x10-5
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