Question

- The binding of glutathione to glutathione S-transferase yields
the following thermodynamic parameters at
288 K: D
_{rxn}G^{o}= -20.7 kJ/mol, D_{rxn}H^{o}= -10.9 kJ/mol, D_{rxn}S^{o}=34.0 J mol^{-1}K^{-1}, D_{rxn}C_{p}^{o}= -912.5 J mol^{-1}K^{-1}Determine the enthalpy and entropy of reaction at 310 K. Assume constant pressure.

Answer #1

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...

9. Consider the ribonuclease folding reaction,
U → F
Experimental measurements indicate the following thermodynamic
parameters (T=298K):
ΔGo'
(kJ/mol)
ΔHo'
(kJ/mol)
ΔSo'
(J/K∙mol)
-46
-280
-790
Calculate the equilibrium constants at T=298K and T=310K.
K298 = ________
K310 = ________

he thermodynamic properties for a reaction are related by the
equation that defines the standard free energy, ΔG∘, in
kJ/mol:
ΔG∘=ΔH∘−TΔS∘
where ΔH∘ is the standard enthalpy change in kJ/mol and
ΔS∘ is the standard entropy change in J/(mol⋅K). A good
approximation of the free energy change at other temperatures,
ΔGT, can also be obtained by utilizing this
equation and assuming enthalpy (ΔH∘) and entropy
(ΔS∘) change little with temperature.
Part A
For the reaction of oxygen and nitrogen to...

Q1: The entropy of sublimation of a certain compound is 5.2 J
K–1 mol–1 at its normal sublimation point of
72 °C. Calculate the vapour pressure (in torr) of the compound at
33 °C. Assume that the enthalpy of sublimation is constant.
I get 1586.851385 torr
Q2:
Compound
So (J
K–1 mol–1)
A
20
B
96
C
74
D
36
At 298 K, ΔGo is 129 kJ / mol for the
reaction
3A + 2B == 2C + 2D
Calculate...

4. Thermodynamic data for C(graphite) and
C(diamond) at 298 K is given in the table
below.
delta Hfo (kJ/mol)
o (J/mol K
C(graphite)
0.0
5.740
C(diamond)
1.895
2.377
a) Calculate delta Ho and delta So and
delta Go for the transformation of 1 mole of graphite
to diamond at 298 K.
b) Is there a tempature at which this transformation will occur
spontaneously at atmospheric pressure? Justify your answer.
8. Methanol can be made using the Fischer-Tropsch process
according to...

Consider the following reaction at 195 K:
2Cu2O (s) ----> 4 Cu (s) + O2 (g)
In one of your laboratory experiments, you determine the
equilibrium constant for this process, at 195 K, is 5.060E-84. You
are given a table of data that indicates the standard heat of
formation (deltaHform) of Cu2O is -170 kJ/mol. Based on this
information, what is the stnadard entropy change (deltaSrxn) for
this reaction at 195 K? (answer in J/K). Show all work please!

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?

HgO(s)
Hg(g)
O2(g)
Enthaply Delta H kj/mol
-90.8
61.3
Entropy Delta S j/mol. K
70.3
174.9
205.0
Above is a table of thermodynamics date for the chemical species
in the reaction: 2HgO(s) ----> 2Hg(g)+ O2(g) at 25 C
A) Calculate the molar entropy of reaction at 25 C
B) Calculate the standard Gibbs free enregy of the reaction at
25 C given that the enthaply of reaction at 25 C is 304.2
Kj/mol
C)Calculate the equilibrium constant for the reaction...

For the following reaction dHorxn= 63.11
kJ/mol and dSorxn= 148 J/mol K.
BaCl2H2O(s) <--->
BaCl2(s) + H2O(g)
a) Write out the equilibrium constant for the reaction and use
it to calculate the vapor pressure of the gaseous water
(PH2O) avoe the BaCl2
H2O at 298K.
b) Assuming dHorxn and
dSorxn are temperature independent estimate
the temperature at which the quilibrium constant (and the
PH2O) = 1bar.

1) Given the following thermochemical reaction and thermodynamic
data, find Gibbs Free Energy, ΔG, and determine if the reaction is
spontaneous or non-spontaneous at 25 °C?
N2(g) + 3H2(g) → 2NH3(g) ΔH = -91.8 kJ
ΔS[N2] = 191 J / mol · K, ΔS[H2] = 131 J / mol · K, and ΔS[NH3]
= 193 J / mol · K
a.98.3 kJ; Non-Spontaneous
b.-98.3 kJ; Spontaneous
c.32.7 kJ; Non-Spontaneous
d.ΔG = -32.7 kJ; Spontaneous
2) What is the oxidation number...

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