Question

Estimate the free energy change (?Grxn) for the following reaction at 298 K, if each gaseous substance is present at p = 0.55 atm (in kJ).

C2H5OH(l) + 3O2(g) ? 2CO2(g) + 3H2O(l)

Answer #1

Estimate the free energy change (?Grxn) for the
following reaction at 298 K, if each gaseous substance is present
at p = 0.25 atm.
C2H5OH(l) + 3O2(g) ?
2CO2(g) + 3H2O(l)
Enter your answer in kJ.

For a gaseous reaction, standard conditions are 298 K and a
partial pressure of 1 atm for all species.
For the reaction
C2H6(g)+H2(g)↽−−⇀2CH4(g)
the standard change in Gibbs free energy is Δ?°=−69.0 kJ/mol.
What is ΔG for this reaction at 298 K when the partial
pressures are ?C2H6=0.300 atm, ?H2=0.500 atm, and ?CH4=0.950
atm?

Calculate Grxn at 298 K under the conditions shown below for the
following reaction.
3 O2(g) ? 2 O3(g); ?G� = +326 kJ
P(O2) = 5.2 atm, P(O3) = .14 atm
Is this reaction spontaneous? Explain and show all work.

For the reaction below, which of the following statements
is(are) true? C2H5OH(l) + 3O2(g) →2CO2(g) + 3H2O(l) ΔH= –1.37 x 103
kJ/mol
I. The reaction is exothermic. II. The enthalpy change would be
different if gaseous water were produced. III. The reaction is not
an oxidation–reduction reaction.

Diamond
a. At 298 K, what is the Gibbs free energy change G for the
following reaction? Cgraphite -> Cdiamond
b. Is the diamond thermodynamically stable relative to graphite
at 298 K?
c. What is the change of Gibbs free energy of diamond when it is
compressed isothermally from 1 atm to 1000 atm at 298 K?
d. Assuming that graphite and diamond are incompressible,
calculate the pressure at which the two exist in equilibrium at 298
K.
e....

Determine the mass (in grams) of oxygen that will result in a
change in energy of -93.02 kJ when oxygen reacts with excess
ethanol according to the following balanced thermochemical
equation:
C2H5OH(l) + 3O2(g) →
2CO2(g) +
3H2O(l) ΔHr° =
-1367.51 kJ
Report your answer to three significant figures.

1.
Calculate the standard free energy change at 500 K for the
following reaction.
Cu(s) +
H2O(g) à CuO(s) +
H2(g)
ΔH˚f
(kJ/mol)
S˚
(J/mol·K)
Cu(s)
0
33.3
H2O(g)
-241.8
188.7
CuO(s)
-155.2
43.5
H2(g)
0
130.6
2. When
solid ammonium nitrate dissolves in water, the resulting solution
becomes cold. Which is true and why?
a. ΔH˚
is positive and ΔS˚ is positive
b. ΔH˚
is positive and ΔS˚...

A. Using given data, calculate the change in
Gibbs free energy for each of the following reactions. In each case
indicate whether the reaction is spontaneous at 298K under standard
conditions.
2H2O2(l)→2H2O(l)+O2(g)
Gibbs free energy for H2O2(l) is -120.4kJ/mol
Gibbs free energy for H2O(l) is -237.13kJ/mol
B. A certain reaction has ΔH∘ = + 35.4
kJ and ΔS∘ = 85.0 J/K . Calculate ΔG∘ for the
reaction at 298 K. Is the reaction spontaneous at
298K under standard
conditions?

Use the values of ∆Hof given below to
calculate ∆Horxn for the following
reaction:
C2H5OH (l)+ 3O2(g) →
2CO2(g) + 3H2O(g)
Given:
∆Hof (kJ/mol)
C2H5OH (l)
-278
O2(g)
0
CO2(g)
-394
H2O(g)
-242
Use kJ for your answer. ΔHorxn =

consider the following reaction C2H5OH + 3O2 ---> 2CO2 + 3H2O
Calculate the change of enthalpy (delta H).

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