Question

1)A system at equilibrium contains I2(g) at a pressure of 0.10 atm and I(g) at a pressure of 0.16 atm . The system is then compressed to half its volume. A)Find the pressure of I2 when the system returns to equilibrium. Express your answer to two significant figures and include the appropriate units.

i got 0.27 and was wrong

2)Solid carbon can react with gaseous water to form carbon
monoxide gas and hydrogen gas. The equilibrium constant for the
reaction at 700.0 K is *K*p=1.60×10−3.

If a 1.55-L reaction vessel initially contains 153 torr of water
at 700.0 K in contact with excess solid carbon, find the percent by
mass of hydrogen gas of the gaseous reaction mixture at
equilibrium. *m*H2/ *m*H2+*m*CO+*m*H2O
= %

Answer #1

**1)**

**I2 (g) <-----> 2 I (g)
Kp = (pI)^2 / p(I2)
=0.16^2 / 0.10
=0.256**

**when volume become half, pressure will double
I2 (g) <-----> 2 I (g)
0.20 0.32 (initial)
0.20+x 0.32-2x (at equilibrium)
Kp = (pI)^2 / p(I2)
= (0.32-2x)^2 / (0.20+x)
0.256 (0.20+x) = 4x^2 + 0.1024 -1.28 x
0.0512 + 0.256*x = 4x^2 + 0.1024 -1.28 x
4x^2 - 1.536*x + 0.0512 = 0
solving above quadratic equation we get,
x = 0.347 and x=0.0368**

**x can't be 0.347 as in this case pressure of I will
become negative
so,
x = 0.0368
pI2 = 0.20+x = 0.20 + 0.0368 = 0.24 atm
Answer: 0.24 atm**

**I am allowed to answer only 1 question at a
time**

Solid carbon can react with gaseous water to form carbon
monoxide gas and hydrogen gas. The equilibrium constant for the
reaction at 700.0 K is Kp=1.60×10−3. If a 1.55-L reaction vessel
initially contains 247 torr of water at 700.0 K in contact with
excess solid carbon, find the percent by mass of hydrogen gas of
the gaseous reaction mixture at equilibrium.

A system at equilibrium contains I2(g) at a pressure of
0.33 atm and I(g) at a pressure of 0.29 atm . The system
is then compressed to half its volume.
Part A
Find the pressure of I2 when the system returns to
equilibrium.
Part B
Find the pressure of I when the system returns to
equilibrium.

A system at equilibrium contains I2(g) at a pressure
of 0.19 atm and I(g) at a pressure of 0.22 atm . The system is then
compressed to half its volume.
Part A: Find the pressure of I2 when the system returns to
equilibrium
Part B: Find the pressure of I when the system returns to
equilibrium

A system at equilibrium contains I2(g) at a pressure of
0.23 atm and I(g) at a pressure of 0.24 atm . The system
is then compressed to half its volume.
Find the pressure of I2 when the system returns to
equilibrium.
Express your answer to two significant figures and include the
appropriate units.
Find the pressure of I when the system returns to
equilibrium.
Express your answer to two significant figures and include the
appropriate units.

Consider the reaction between iodine gas and chlorine gas to
form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K) A
reaction mixture at 298 K initially contains PI2=0.35 atm and
PCl2=0.35 atm . What is the partial pressure of iodine monochloride
when the reaction reaches equilibrium?

Consider the reaction between iodine gas and chlorine gas to
form iodine monochloride:
I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at
298 K)
A reaction mixture at 298 K initially contains PI2=0.40
atm and PCl2=0.40 atm .
What is the partial pressure of iodine monochloride when the
reaction reaches equilibrium?

Consider the reaction:
H2(g)+I2(g)⇌2HI(g)
A reaction mixture at equilibrium at 175 K contains
PH2=0.958atm, PI2=0.877atm,
and PHI=0.020atm. A second reaction mixture,
also at 175 K, contains
PH2=PI2=0.629
atm , and PHI= 0.101 atm .
Is the second reaction at equillibrium? I found that the
kp=4.76X10-4 and Qp = .0257 So no, not at
equillibrium.
If not, what is the partial pressure of HI when the
reaction reaches equilibrium at 175 K? I need help
figuring out the ICE chart and...

1)A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10
atm ) and O2(P= 1.00 atm ). When a catalyst is added the reaction
2SO2(g)+O2(g)⇌2SO3(g) takes place. At
equilibrium the total pressure is 3.85 atm.
-Find the value of Kc.
2)A sample of SO3 is introduced into an evacuated sealed
container and heated to 600 K. The following equilibrium is
established:
2SO3(g)⇌2SO2(g)+O2(g).
The total pressure in the system is found to be 3.0 atm and the
mole fraction...

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.) The equilibrium constant for the chemical equation
N2(g)+3H2(g) <-->
2NH3(g)
is Kp = 1.09 at 209 °C. Calculate the value of the Kc for the
reaction at 209 °C.
2.) At a certain temperature, 0.3411 mol of N2 and 1.581 mol of
H2 are placed in a 1.50-L container.
N2(g)+3H2(g) <-->
2NH3(g)
At equilibrium, 0.1801 mol of N2 is present. Calculate the
equilibrium constant, Kc.
3.) At a certain temperature, the Kp for the decomposition of
H2S is 0.748....

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