Question

6. If ΔH° for a reaction is +32 kJ and the K_{eq} value
at 25°C is 2.8 x 10^{5} , what is the K_{eq} value
at 100°C?

a. 2.1 x 10^{4}

b. 7.0 x 10^{4}

c. 2.8 x 10^{5}

d. 3.8 x 10^{6}

e. 1.1 x 10^{6}

7. The graph below corresponds to a set of equilibrium constant values, K, measured at different temperatures. What type of reaction must this represent?

Ln K

0

a. A reaction for which ΔH° <0 and ΔS° >0

b. A reaction for which ΔH° =0 and ΔS° =0

c. A reaction for which ΔH° >0 and ΔS° >0

d. A reaction for which ΔH° <0 and ΔS° <0

e. A reaction for which ΔH° >0 and ΔS° <0

8. Indicate which of the following is expected to have the
l**argestt** standard molar entropy (S°).

a. H_{2}O (l)

b. H_{2}O (g)

c. CH_{3}OH(s)

d. H_{2}O (s)

e. CH_{3}OH (l)

Answer #1

1- Calculate ΔG o for the following reaction at 25°C.
You will have to look up the thermodynamic data. 2 C2H6(g) + 7
O2(g) → 4 CO2(g) + 6 H2O(l)
2- A reaction will be spontaneous only at low
temperatures if both ΔH and ΔS are negative. For
a reaction in which ΔH = −320.1 kJ/mol and ΔS =
−99.00 J/K ·mol,determine the temperature (in °C)below which the
reaction is spontaneous.

Please show all work so that i can understand. thank you
A.) Which of the following processes have a ΔS > 0?
a.CH3OH(l) → CH3OH(s)
b.Na2CO3(s) + H2O(g) +
CO2(g) → 2 NaHCO3(s)
c.
CH4(g) + H2O(g) → CO(g) + 3
H2(g)
d.
N2(g) + 3 H2(g) → 2
NH3(g)
e. All of the above processes have a ΔS > 0.
B.) If ΔG > 0, which of the following statements are
true?
a.
The reaction is at equilibrium.
b....

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˚...

Consider the following reaction:
2AgCl(s) → 2Ag(s) +
Cl2(g); ΔH° = 127.1 kJ; ΔS° =
115.7 J/K at 298 K
Suppose 59.4 g of silver(I) chloride is placed in a 63.1 L
vessel at 298 K. What is the equilibrium partial pressure of
chlorine gas? (R = 0.0821 L · atm/(K · mol) = 8.31 J/(K ·
mol))
A.5.7 × 10-17 atm
B.0.95 atm
C.5.1 × 10-23 atm
D.0.081 atm
E.0.16 atm

Calculate the equilibrium constant Keq for the following
reaction at 25°C. (S° values in J/mol•K: N2(g), 191.5 ; O2(g),
205.0 ; Cl2(g), 223.0 ; NOCl(g), 261.6) N2(g) + O2(g) + Cl2(g) ↔
2NOCl(g) ΔH° = 103.4 kJ
a. 2.43 x 10−20
b. 8.82 x 10−29
c. 5.91 x 10−17
d. 2.01 x 10−10
e. 6.99 x 10−24

Predict the sign of the entropy change, ΔS∘, for each of the
reaction displayed. Explain your Reasoning for each.
A. CH3OH(l) --> CH3OH(s)
B. N2(g) + 3H2(g) --> 2NH3(g)
C. CH4(g) + H2O(g) --> CO(g) + 3H2(g)
D. 2HBr(g) --> H2(g) + Br2(l)

For a certain reaction, ΔH°=−14.6 kJ and ΔS°=−233 J/K.
If n=2, calculate E°cell for the reaction at 25°C.
a. −0.284 V
b. 0.0961 V
c. −0.130 V
d. 0.736 V
e. 0.0654 V

Calculate the standard cell potential at 25 ∘C for the
reaction
X(s)+2Y+(aq)→X2+(aq)+2Y(s)
where ΔH∘ = -793 kJ and ΔS∘ = -143 J/K .

Calculate the standard cell potential at 25 ∘C for the reaction
X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -597 kJ and ΔS∘ = -337
J/K

please finish the whole thing, ( Thank you )
a. For a certain chemical reaction, ΔH = - 34.4 kJ and
ΔS = - 85.0 J/K
Calculate ΔG or the reaction at 298K
b. By using data in Appendix E in the textbook, determine which
is the more unfavorable reduction, Cd2+ (aq) to Cd(s) or
Ca2+ (aq) to Ca(s).
c. Using standard reduction potentials (Appendix E in the
textbook), calculate the standard emf for each of the following
reactions.
2Al3+(aq)+3Ca(s)→2Al(s)+3Ca2+(aq)...

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