Question

1. The reaction I2(g) + Cl2(g) ⇔ 2 ICl(g) is at equilibrium when the partial pressures are: I2 = 0.027 atm, Cl2 = 0.027 atm and ICl = 0.246 atm. The partial pressure of ICl is then increased to 0.500 atm by adding ICl.

a. When the system re-establishes equilibrium, what is the partial pressure of Cl2(g)?

b. When the system re-establishes equilibrium, what is the partial pressure of ICl(g)

c. When the system re-establishes equilibrium, what is the partial pressure of I2(g)

2. 2 NaHCO3(s) ⇔ Na2CO3(s) + H2O(g) + CO2(g) enthalpy = +128 kJ is at equilibrium.

a. What happens to [Na2CO3(s)] when NaHCO3 is added?

b. What happens to Kc when the temperature increases?

c. What happens to [CO2] when the H2O is added?

d. What happens to the value of Kp when Na2CO3 is added?

Answer #1

Equilibrium constant doesn't depend upon pressure.

4) At a certain temperature, Kp for the reaction, Cl2(g) + I2(g)
<=> 2 ICl(g) is 3,230.
Calculate the value of Kp for the reaction, 1/2 Cl2(g) + 1/2
I2(g) <=> ICl(g)
5) Calculate Kc for the following reaction,
H2(g) + I2(g) <=> 2 HI(g);
Kp = 97.5 at 25.0 o C

Consider reaction
I2(g)+Cl2(g)<======>2ICL(g) Kp=81.9 at 25 C
A mixture at 25 C initially contains Pcl12=0.100 atm
PI2=0.100 PICl=0.100
Find the equilibrium partial pressures of
I2,Cl2,and ICL at this temp.
I want to know how to slove this problem with ICE table and show
tips and ways around thanks.

At 1000 K, Kp = 19.9 for the reaction
Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g).
What are the equilibrium partial pressures of CO and CO2 if CO
is the only gas present initially, at a partial pressure of 0.940
atm ?

At 400K, the equilibrium constant for the reaction I2(g) + F2(g)
<==> 2 IF (g) Kp = 7.0. A closed vessel at 400 K is charged
with 1.46 atm I2, 1.46 atm F2, and 3.66 atm of IF. Which of the
following statements is true? CAN YOU PLEASE EXPLAIN WHY?
THANK YOU!
A. The equilibrium partial pressures of I2 F2, and IF will not
change.
B. At equilibrium, the total pressure of IF wil be greater than
3.66 atm.
C....

1-Calculate the partial pressure (in atm) of Cl2 at
equilibrium when 4.38 atm of COCl2 dissociates at 350 K
according to the following chemical equilbrium:
COCl2(g) ⇌ CO(g) + Cl2(g)
Kp = 8.77×10-10
***If the 5% approximation is
valid, use the assumption to compute the partial pressure. Report
your answer to three significant figures in scientific
notation.
2-Calculate the partial pressure (in atm) of
CH3OH at
equilibrium when 4.84 atm of CH3I and 4.84 atm of
H2O react at 3000...

1) The equilibrium constant, Kp, for the following
reaction is 0.497 at 500 K:
PCl5(g) <---
----->PCl3(g) +
Cl2(g) (reversible)
Calculate the equilibrium partial pressures of all species when
PCl5(g) is introduced into an evacuated
flask at a pressure of 1.52 atm at
500 K.
PPCl5
=
_____atm
PPCl3
=
______atm
PCl2
=
______atm
2) The equilibrium constant, Kp, for the following
reaction is 55.6 at 698 K:
H2(g) +
I2(g) <----- ---->
2HI(g) (reversible)
Calculate the equilibrium partial pressures...

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?

The equilibrium constant Kp for the reaction
C(s)+H2O(g)?CO(g)+H2(g) is 2.44
at 1000 K. What are the equilibrium partial pressures of H2O, CO,
and H2 if the initial partial pressures are PCO= 1.25 atm,
and PH2= 1.60 atm?
What is the equilibrium partial pressure of H2O?
What is the equilibrium partial pressure of CO?
What is the equilibrium partial pressure of H2?

Consider the reaction.
A(g)⇌2B(g)
Find the equilibrium partial pressures of A and Bfor each of the
different values of Kp. Assume that the initial partial
pressure of B in each case is 1.0 atm and that the initial partial
pressure of A is 0.0 atm. Make any appropriate simplifying
assumptions.
Part A
Kp= 2.4
Part B
Kp= 1.9×10−4
Part C
Kp= 1.8×105

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has
partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr,
respectively. A quantity of Cl2(g) is injected into the mixture,
and the total pressure jumps to 263.0 Torr (at the moment of
mixing). The system then re-equilibrates. The appropriate chemical
equation is

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