Question

When 0.0430 mol of HI is heated to 500 K in a 5.00 L sealed container, the resulting equilibrium mixture contains 2.85 g of HI. Calculate Kc and Kp for the following decomposition reaction. 2 HI (g) H2 (g) + I2 (g)

Answer #1

2 HI (g) H_{2
(}g) + I_{2} (g).

Kc = [HI]^{2} HI moles = 0.0430, the volume
= 5L

HI concentration (Molarity) = Moles/ litre

= 0.0430/5

= 0.0086M.

Kc = [0.0086]^{2}

**Kc = 7.396 x 10 ^{-5}.**

Kp = Kc[RT]^{n}
R = Ideal gass constant = 8.314
jk^{-1}mol^{-1.}

^{ } n = Gaseous
product mole no - gaseous reactant mol no.

n = 2-2

n = 0

Kp = Kc[RT]^{n} T = 500 K
(according to the question).

Kp = 7.396 x 10^{-5}[8.314x500]^{0}

Kp = 7.396 x 10^{-5.}

A sample of HI (9.30 x 10-3 mol) was placed in an empty 2.00 L
container at 1000 K. After equilibrium was reached, the
concentration of I2 was 6.29 x 10- 4 M. Calculate the value of Kc
at 1000 K for the reaction H2(g) + I2(g) 2HI(g).

1. Consider 1.20 mol of carbon monoxide and 4.00 mol of chlorine
sealed in a 6.00 L container at 476 oC. The equilibrium constant,
Kc, is 2.50 (in M-1) for
CO(g) + Cl2(g) ? COCl2(g)
Calculate the equilibrium molar concentration of CO.
2. For the reaction in the previous problem, that is,
2HI(g) ? H2(g) + I2(g) Keq = 0.016
Initially a container contains 0.40 M HI and no product. What is
the equilibrium concentration of H2?

A 1.00 L container holds 0.015 mol of H2 (g) , 0.015 mol of I2
(g), and 0.015 mol of HI (g) at 721 K. What are the
concentrations(pressures) of H2 (g), I2 (g), and HI (g) after the
system achieved a state of equilibrium? The value of Kc is 50.0 for
reaction: H2 (g) + I2 (g) 2HI (g)

At 400 K, an equilibrium mixture of H2, I2, and HI consists of
0.082 mol H2, 0.084 mol I2, and 0.15 mol HI in a 2.50-L flask. What
is the value of Kp for the following equilibrium? (R = 0.0821 L ·
atm/(K · mol))
2HI(g) H2(g) + I2(g)
A. 0.045
B. 7.0
C. 22
D. 0.29
E. 3.4

A quantity of HI was sealed in a tube, heated to 425°C, and held
at this temperature until equilibrium was reached. The
concentration of HI in the tube at equilibrium was found to be
0.0706 moles/liter. Calculate the equilibrium concentration of
H2 (and I2). (Hint: H2 and
I2 are equal).
For the
reaction:
H2(g) + I2(g) ßà 2
HI(g)
Kc = 54.6 at 425°C.
a. 4.78 × 10-3M
b. 9.55 × 10-3M
c. 2.34 × 10-3M
d. 1.17 ×...

An equilibrium mixture contains 0.710 mol HI, 0.460 mol I2, and
0.250 mol H2 in a 1.00-L flask.
What is the equilibrium constant for the following reaction?
2HI(g) H2(g) + I2(g)
K =
How many moles of I2 must be
removed in order to double the number of moles of H2 at
equilibrium?
_______ mol I2

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?

A mixture of water and graphite is heated to 890 K in a 10.0-L
container. When the system comes to equilibrium it contains 0.895
mol each of H2 and CO and 0.302 mol of H2O and some graphite. Some
O2 is added to the system and a spark is applied so that the H2
reacts completely with the O2, forming H2O. Find the amount of CO
in the flask when the system returns to equilibrium.

When 1.10 mol CO2 and 1.10 mol H2 are placed in a 3.00-L
container at 395 ∘C, the following reaction occurs:
CO2(g)+H2(g)⇌CO(g)+H2O(g).
A. If Kc = 0.802, what are the concentrations
of CO2 in the equilibrium mixture?

A sample of CaCO3(s) is introduced into a sealed container of
volume 0.674 L and heated to 1000 K until equilibrium is reached.
The Kp for the reaction CaCO3(s)⇌CaO(s)+CO2(g) is 3.9×10−2 at this
temperature. Calculate the mass of CaO(s) that is present at
equillibrium.
please show work

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