Question

The equation for the formation of hydrogen iodide from
H_{2} and I_{2} is:

H_{2}(g) + I_{2}(g) <--> 2HI(g)

The value of K_{p} for the reaction is 69.0 at 730.0C.
What is the equilibrium partial pressure of HI in a sealed reaction
vessel at 730.0C if the initial partial pressures of H_{2}
and I_{2} are both 0.1600 atm and initially there is no HI
present?

Answer #1

write out the Kp expression, where Pp is the partial
pressure:

Kp = (Pp HI^2)/(Pp H2 * Pp I2)

Pp H2 = Pp I2 =0.016 atm

Let the partial pressure of HI at equilibrium is x

So

69.0 = (x)^2/(0.16 * 0.16)

=> x^{2} = 69 / 0.16*0.16

=> **x = 1.329 atm**

. To check, plug the equilibrium pressure back into the Kp
expression, making sure that you get close to the Kp value you were
given. If you do, you know it's correct.

Kp = 68.993 by putting the va;ue back in the equation

Hydrogen iodide decomposes according to the equation 2HI
(g)<---> H2 (g) + I2 (g) for which K= .0156 at 400 degrees
celsius. If 0.550 mol of HI was injected into 2.00L reaction vessel
at 400 degrees celsuis. Calculate the concentration of H2 at
equilibrium?

Kc for the reaction of hydrogen and
iodine to produce hydrogen iodide.
H2(g) + I2(g) ⇌
2HI(g)
is 54.3 at 430°C. Calculate the
equilibrium concentrations of H2,
I2, and HI at 430°C if
the initial concentrations are [H2] =
[I2] = 0 M,
and [HI] = 0.483 M.

Kc for the reaction of hydrogen and iodine to produce hydrogen
iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430 ° C. Calculate the
equilibrium concentrations of H2, I2, and HI at 430 ° C if the
initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.445
M.

Hydrogen iodide, HI, decomposes at moderate temperature
according to the equation 2HI (g) H2 (g) + I2 (g) When 4.00 mol HI
was placed in a 5.00-L vessel at 458C, the equilibrium mixture was
found to contain 0.442 mol I2. What is the value of Kc for the
decomposition of HI at this temperature?

Hydrogen iodide undergoes decomposition according to the
equation 2HI(g) H2(g) + I2(g) The equilibrium constant Kp at 500 K
for this equilibrium is 0.060. Suppose 0.898 mol of HI is placed in
a 1.00-L container at 500 K. What is the equilibrium concentration
of H2(g)?
(R = 0.0821 L · atm/(K · mol))
A. 7.3 M
B. 0.40 M
C. 0.15 M
D. 0.18 M
E. 0.043 M

Hydrogen iodide decomposes according to the following reaction.
2 HI(g) equilibrium reaction arrow H2(g) + I2(g) A sealed 1.5 L
container initially holds 0.00615 mol H2, 0.00445 mol I2, and
0.0163 mol HI at 703 K. When equilibrium is reached, the
equilibrium concentration of H2(g) is 0.00364 M. What are the
equilibrium concentrations of HI(g) and I2(g)?

An equilibrium mixture for the following reaction: H2(g) + I2(g)
<---> 2HI(g) is composed of the following: P(I2) = 0.08592
atm; P(H2) = 0.08592 atm; P(HI) = 0.5996 atm. If this equilibrium
is disturbed by adding more HI so that the partial pressure of HI
is suddenly increased to 1.0000 atm, what will the partial
pressures of each of the gases be when the system returns to
equilibrium?

CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are
allowed to react in a sealed vessel at 464 ∘C . At equilibrium, the
concentrations were measured and the following results obtained:
Gas Partial Pressure (atm) CO 0.780 Cl2 1.22 COCl2 0.120 What is
the equilibrium constant, Kp, of this reaction? Part B The
following reaction was performed in a sealed vessel at 767 ∘C :
H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at
concentrations of [H2]=3.75M and [I2]=2.05M. The equilibrium
concentration...

H2
+ I2 <---> 2HI
Kp=100
Initially, a flask contains hydrogen gas at 0.010atm iodine
gas at 0.0050atm, and hydorgen iodide gas at 0.50atm.
Determine equilibrium partial pressure of each gas in the
flask.

The system
H2(g) + I2(g) ⇌ 2HI(g
) is at equilibrium at a fixed temperature with a partial
pressure of H2 of 0.200 atm, a partial pressure of I2 of 0.200 atm,
and a partial pressure of HI of 0.100 atm. An additional 0.26 atm
pressure of HI is admitted to the container, and it is allowed to
come to equilibrium again. What is the new partial pressure of
HI?
A.0.360 atm
B. 0.464 atm
C. 0.152 atm
D. 0.104...

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