Question

1-Calculate the partial pressure (in atm) of Cl_{2} at
equilibrium when 4.38 atm of COCl_{2} dissociates at 350 K
according to the following chemical equilbrium:

COCl_{2}(g) ⇌ CO(g) + Cl_{2}(g) |
K_{p} = 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
CH_{3}OH at
equilibrium when 4.84 atm of CH_{3}I and 4.84 atm of
H_{2}O react at 3000
K according to the following chemical equation:

CH_{3}I (g) + H_{2}O (g) ⇌ CH_{3}OH (g)
+ HI (g) |
K_{p} = 7.47×10^{1} |

****Report your answer to three
significant figures in scientific notation.

Answer #1

1. let x be the change in partial pressure of COCL2 at equilibrium

Kp = [CO][Cl2]/[COCl2]

8.77 x 10^-10 = x^2/4.38

Thus partial pressure of Cl2 at equilibrium (x) = 6.198 x 10^-5 atm

2. let x be the change in partial pressures of CH3I and H2O at equilibrium

Kp = [CH3OH][HI]/[CH3I][H2O]

7.47 x 10^1 = x^2/(4.84 - x)(4.84 - x)

1749.8923 + 7.47 x 10^1x^2 - 723.096x = x^2

73.7x^2 - 723.096x + 1749.8923 = 0

x = 0.0676 atm

Thus, partial pressure of CH3OH at equilibrium = 6.766 x 10^-2 atm

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 K according to the following chemical
equation:
CH3I (g) + H2O (g) ⇌ CH3OH (g)
+ HI (g)
Kp = 7.47×101
Report your answer to three significant figures in scientific
notation.
**** i have just one chance !!

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 K according to the following chemical
equation:
CH3I (g) +
H2O (g) ⇌ CH3OH (g) + HI (g)
Kp =
7.47×101
Report your answer to three significant figures in scientific
notation.
**** i have just one chance !!

1-Calculate the partial pressure (in atm) of H2O at
equilibrium when 59.6 g of CdO and 3.21 atm of H2 react
at 800 K according to the following chemical equation:
CdO(s) + H2(g) ⇌ Cd(s) + H2O(g)
Kp = 4.12×101
***Report your answer to three
significant figures in scientific notation.
2-Calculate the partial pressure (in atm) of H2O at
equilibrium when 1.38 atm of CH3OH and 6.77 atm of HCl
react at 2000 K according to the following chemical equation:...

Calculate the partial pressure (in atm) of C2H5Br at equilibrium
when 1.23 atm of C2H6 and 6.21 atm of Br2 react at 2500 K according
to the following chemical equation:
C2H6 (g) + Br2 (g) ⇌ C2H5Br (g) + HBr (g) Kp = 6.87
Report your answer to three significant figures in scientific
notation.

A mixture containing C5H6, HCl, Cl2, and C5H8, all at an initial
partial pressure of 4.95 atm, is allowed to achieve equilibrium
according to the equation below. At equilibrium, the partial
pressure of C5H8 is observed to have decreased by 0.37 atm.
Determine Kp for this chemical equilibrium. Report your answer
to 3 significant figures in scientific notation.
C5H6(g) + 2HCl(g) ⇌ Cl2(g) + C5H8(g)

A mixture containing HF, F2, and H2, all
at an initial partial pressure of 2.69 atm, is allowed to achieve
equilibrium according to the equation below. At equilibrium, the
partial pressure of H2 is observed to have increased by
0.13 atm. Determine Kp for this chemical equilibrium.
Report your answer to 3 significant figures in scientific
notation.
2HF(g) ⇌ F2(g) + H2(g)

A mixture containing C5H6, HBr, Br2, and C5H8, all at an initial
partial pressure of 1.47 atm, is allowed to achieve equilibrium
according to the equation below. At equilibrium, the partial
pressure of C5H8 is observed to have decreased by 0.90 atm.
Determine Kp for this chemical equilibrium. Report your answer to 3
significant figures in scientific notation.
C5H6(g) + 2HBr(g) ⇌ Br2(g) + C5H8(g)

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...

The equilibrium
2NO(g)+Cl2(g)⇌2NOCl(g)
is established at 500 K. An equilibrium mixture of the three gases
has partial pressures of 9.50×10−2 atm , 0.174 atm , and
0.27 atm for NO, Cl2, and NOCl, respectively.
Part A
Calculate Kp for this reaction at 500.0 K.
Express your answer using two significant figures.
Part B
If the vessel has a volume of 5.80 L, calculate
Kc at this temperature.
Express your answer using two significant figures.
.

A gas mixture consists of 4.45 atm of Cl2O, 4.14 atm
of O2, 0.784 atm of Cl2, and 0.14 atm of
O3.
1-Calculate the reaction quotient for this system prior to the
establishment of the equilibrium below.
Cl2(g) + O3(g) ⇌ Cl2O(g) + O2(g)
***Report your answer to three significant figures in scientific
notation.
2-If the equilibrium constant for this reaction at 3000 K is
5.65, determine the direction that the reaction will shift in order
to achieve equilibrium.

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