Question

Estimate the value of the equilibrium constant at 625 K for each of the following reactions. ΔH∘f and S∘ for BrCl(g) is 14.6 kJ/mol and 240.0 Jmol⋅K, respectively. Part A 2NO2(g)⇌N2O4(g) Please be fast because it will soon be over by 11:59pm. Thank you

Answer #1

Part A

2NO2(g) <--------------> N2O4(g)

ΔH∘rxn = ΔH∘f products - ΔH∘f reactants

= 11.1 - (2 x 33.2)

= - 55.3 kJ/mol

ΔSorxn = 304.4 - (2 x 240.1)

= - 175.8 J/K

ΔGo = ΔH∘ - T ΔSo

= - 55.3 - 625 x (- 0.1758)

= 54.58 kJ/mol

ΔGo = - RT ln K

54.58 = - 8.314 x 10^-3 x 625 x ln K

K = 2.75 x 10^-5

**Equilibrium constant K = 2.75 x 10^-5**

Estimate the value of the equilibrium constant at 530 K for each
of the following reactions. 2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 550 K for each
of the following reactions.
a) 2CO(g)+O2(g)⇌2CO2(g)
b) 2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 525 K for each
of the following reactions.
A.
2CO(g)+O2(g)⇌2CO2(g)
B.
2H2S(g)⇌2H2(g)+S2(g)

Estimate the value of the equilibrium constant at 525 K for each
of the following reactions.
A. 2CO(g)+O2(g)⇌2CO2(g)
B. 2H2S(g)⇌2H2(g)+S2(g)

Enter your answer in the provided box. For reactions carried out
under standard-state conditions, the equation ΔG = ΔH − TΔS becomes
ΔG o = H o − TΔS o . Assuming ΔH o and ΔS o are independent of
temperature, one can derive the equation: ln K2 K1 = ΔH o R ( T2 −
T1 T1T2 ) where K1 and K2 are the equilibrium constants at T1 and
T2, respectively. Given that at 25.0°C, Kc is 4.63 ×...

Use the thermodynamic data below to determine the equilibrium
constant for the conversion of oxygen to ozone at 3803°C
3O2 (g) ⇌ 2O3
(g)
substance ΔH˚f
(kJ/mol) ΔG˚f
(kJ/mol) S˚ (J/mol*K)
O2
(g) 0 0 205.0
O3
(g) 142.3
163.4
237.6

1. The equilibrium constant, Kp, for the following reaction is
4.55×10-5 at 723 K.
N2(g) + 3H2(g) 2NH3(g)
If ΔH° for this reaction is -111 kJ, what is the value of Kp at
839 K?
Kp=
2. The equilibrium constant, Kp, for the following
reaction is 0.110 at 298 K.
NH4HS(s)
NH3(g) +
H2S(g)
If ΔH° for this reaction is 92.7 kJ, what is the
value of Kp at 393 K?
Kp=

Use the free energies of formation given below to calculate the
equilibrium constant (K) for the following reaction at 298 K.
2 HNO3(aq) + NO(g) → 3 NO2(g) +
H2O(l) K = ?
ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
Calculate the ΔG∘rxn for the reaction using the following
information.
4HNO3(g)+5N2H4(l)→7N2(g)+12H2O(l)
ΔG∘f(HNO3(g)) = -73.5 kJ/mol;
ΔG∘f(N2H4(l)) = 149.3 kJ/mol;
ΔG∘f(N2(g)) = 0 kJ/mol;
ΔG∘f(H2O(l)) = -273.1 kJ/mol.
Calculate the ΔG°rxn using the following
information.
2 H2S(g) + 3 O2(g) → 2...

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following reactions at equilibrium cause the system to shift in the
direction of the products or the reactants?
Part A
2NH3(g)???3H2(g)+N2(g)
A. Increasing the volume will shift the system in the direction
of the products.
B. Increasing the volume will shift the system in the direction of
the reactants.
C. Increasing the volume will not shift the equilibrium.
Part B
N2(g)+O2(g)???2NO(g)
A. Increasing the volume will shift the system...

Question 1:
The reaction 2CH4(g)⇌C2H2(g)+3H2(g) has an equilibrium constant of K =
0.154. If 6.25 mol of CH4,
4.45 mol of C2H2, and 11.55 mol of H2 are added to a reaction
vessel with a volume of 6.00 L , what net reaction will occur-
answer a, b or c?
a) The reaction will proceed to the left to establish
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