Question

Consider the reaction, Ag_{2}CO_{3}(s) ↔
Ag_{2}O(s) + CO_{2}(g), for which the following
data have been reported for the equilibrium constant
(K_{eq}) measured at four different temperatures:

T = 350 K 400 K 450 K 500 K

K_{eq}
= 3.98 x
10^{-4}
1.41 x 10^{-2}
1.86 x
10^{-1}
1.48

**(a).** Does this data indicate that the reaction
is endothermic or exothermic? Give a rationale for your answer.

**(b).** Can this data be used to calculate a value
for the ∆_{r}H^{o} of the reaction? If you answer
Yes, explain how you would go about doing that.

Answer #1

a)

First, analyse the trend as T increases... this implies the system gets more ENERGY

As T increases, Keq increases as well

this implies:

Keq = [Products] / [reactants]

now, as K increases, this implies [Products] /increases and [reactants] decreases

therefore, this must be ENDOTHERMIC

that is, as we add more energy, the equilibrium favours the products

b)

Yes, this could be done, we must apply vant Hoff equation

it relates:

ln(K) = -H/R*(1/T) + S/R

in which we can fit many data as follows:

ln(K2/K1) = -H/(R) * (1/T2 - 1/T1)

Consider the following reaction: CaCO3(s)→CaO(s)+CO2(g) Estimate
ΔG∘ for this reaction at each of the following temperatures.
(Assume that ΔH∘ and ΔS∘ do not change too much within the given
temperature range.)
Part A
315 K
Express your answer using one decimal place.
ΔG∘ =
kJ
Part B
1075 K
Express your answer using one decimal place.
ΔG∘ =
kJ
Part C
1440 K
Express your answer using one decimal place.
ΔG∘ =
kJ

Consider the following reaction:
CaCO3(s)→CaO(s)+CO2(g).
Estimate ΔG∘ for this reaction at each of the following
temperatures. (Assume that ΔH∘ and ΔS∘ do not
change too much within the given temperature range.)
A. 1090 K
B.1405 K
C.Predict whether or not the reaction in part A will be
spontaneous at 320 K .
D. Predict whether or not the reaction in part B will be
spontaneous at 1090.
E. Predict whether or not the reaction in part C will be
spontaneous...

Consider the following reaction:
PbCO3(s)←−→PbO(s)+CO2(g)
Part A: Using data in Appendix C in the textbook, calculate the
equilibrium pressure of CO2 in the system at 440 ∘C. Express your
answer using two significant figures.
Part B: Using data in Appendix C in the textbook, calculate the
equilibrium pressure of CO2 in the system at 250 ∘C. Express your
answer using two significant figures.

Consider the following reaction:
PbCO3(s)←−→PbO(s)+CO2(g)
Part A
Using data in Appendix C in the textbook, calculate the
equilibrium pressure of CO2 in the system at 440 ∘C.
Express your answer using two significant figures.
PCO2 =
atm
Part B
Using data in Appendix C in the textbook, calculate the
equilibrium pressure of CO2 in the system at 250 ∘C.
Express your answer using two significant figures.
PCO2 =
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

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