Question

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*)

Answer #1

a) 2CO(g) + O2(g) <-------> 2CO2(g)

∆G° = ∆G°f(Products) - ∆G°f(Reactants)

= (2×∆H°f(CO2) ) - ( 2×∆H°f(CO) + ∆H°f(O2))

= ( 2× ( -394.39kJ/mol) ) - ( 2 × (-137.6kJ/mol) + 0 )

= -788.78kJ/mol + 275.2kJ/mol

= -513.6kJ/mol

∆G° = - RTlnK

-513.6kJ/mol = - 8.314(J/K mol) × 550K× 2.303logK

logK = 513.6/10.53

= 48.77

K = 5.9 × 10^48

b) 2H2S(g) <-------> 2H2(g) + S2(g)

∆G°= (∆G°f(H2) + ∆G°(S2) ) - ( 2× H2S))

= ( 0 + 0 ) - ( 2× (-21kJ/mol))

= + 42kJ/mol

∆G° = - RTlnK

42kJ/mol = - ( 8.314 × 550K × 2.303 × logK)

logK =-( 42/10.53)

= -3.99

K = 1.02×10^-4

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)

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

Use data from Appendix IVB to calculate the equilibrium
constants at 25∘C for each reaction. Express your answer using two
significant figures.
Part A: 2CO(g)+O2(g)⇌2CO2(g)
Part B: 2H2S(g)⇌2H2(g)+S2(g)

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

What would be the effect of increasing the volume on each of the
following reactions at equilibrium (shift left, shift right, or no
change)?
A) 2CO (g) + O2 (g) <-----> 2CO2
(g)
B) N2O4 (g) <-----> 2NO2
(g)

A gas phase that is at equilibrium with respect to the following
reaction at 500 K contains carbon dioxide, carbon monoxide, and
oxygen.
2CO2(g) → 2CO(g) +
O2(g)
a) Calculate the equilibrium partial pressure of oxygen if the
carbon dioxide partial pressure is 0.20 atm and the carbon monoxide
partial pressure is 0.40 atm. The ∆G°f values for
CO2 and CO at 500 K are -94.389 kcal/mol and -37.140
kcal/mol, respectively.
b) Calculate the total pressure at equilibrium if the...

Which equation is matched with the correct equilibrium
expression for that reaction?
Which equation is matched with the correct equilibrium
expression for that reaction?
O3(g) + O(g) →
2O2(g), K c = 2 ×
[O2]/[O3][O]
2CO(g) + O2(g) →
2CO2(g), K c =
[CO2]/[CO][O2]
2CO2(g) → 2CO(g)
+ O2(g) K c =
[CO2]2/[CO]2[O2]
N2(g) + O2(g)
→ 2NO(g), K c =
[NO]2/[N2][O2]
Calculate the pH for an aqueous solution of acetic acid that
contains 5.15 × 10-3 hydronium ion.
Calculate...

Consider the following reaction at equilibrium:
2H2(g)+S2(g)⇌2H2S(g)+heat
In a 10.0-L container, an equilibrium mixture contains 2.20 g of
H2, 10.9 g of S2 and 68.1 g of H2S.
Part A What is the numerical Kc value for this
equilibrium mixture?
Part B If more H2 is added to the equlibrium mixture, how will
the equilibrium shift?
Part C How will the equilibrium shift if the mixture is placed
in a 5.00-L container with no change in temperature?
Part D If...

A.) Express the equilibrium constant for the combustion of
ethane in the balanced chemical equation.
2C2H6(g)+7O2(g)⇌4CO2(g)+6H2O(g)
K=[C2H6]2[O2]7 / [CO2]4[H2O]6
K=[CO2]4 / [C2H6]2[O2]7
K=K=[CO2]4[H2O]6 / [C2H6]2[O2]7
K=[CO2][H2O] / [C2H6]2[O2]
B.)Consider the chemical equation and equilibrium constant at
25∘C:
H2(g)+I2(g)⇌2HI(g) , K=6.2×102
Calculate the equilibrium constant for the following reaction at
25∘C:
HI(g)⇌12H2(g)+12I2(g)
Express the equilibrium constant to two significant figures.
C.) Consider the following reaction and corresponding value of
Kc:
H2(g)+Br2(g)⇌2HBr(g) , Kc=1.9×1019 at 25∘C
What is the value of Kp...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 2 minutes ago

asked 2 minutes ago

asked 2 minutes ago

asked 19 minutes ago

asked 23 minutes ago

asked 29 minutes ago

asked 30 minutes ago

asked 30 minutes ago

asked 38 minutes ago

asked 42 minutes ago

asked 43 minutes ago