Chapter 14:Chemical Equilibrium

Example no:14.2,Page no:622

In [20]:
#Variable declaration
NO=0.0542 #equilibrium conc of NO, M
O2=0.127 #equilibrium conc of O2, M
NO2=15.5 #equilibrium conc of NO2, M

#Calculation
Kc=NO2**2/(O2*NO**2) #equilibrium constant for given reaction

#Result
print"The value of the equilibrium constant of the reaction is %.2e"%Kc

The value of the equilibrium constant of the reaction is 6.44e+05

Example no:14.3,Page no:623

In [5]:
#Variable declaration
PCl3=0.463 #equilibrium pressure of PCl3, atm
PCl5=0.875 #equilibrium pressure of PCl5, atm
Kp=1.05 #equilibrium constant of the reaction

#Calculation
Cl2=Kp*PCl5/PCl3 #equilibrium pressure of Cl2 in atm, formula from the definition of equilibrium constant

#Result
print"The value of the equilibrium pressure of the Cl2 gas is :",round(Cl2,2),"atm"

The value of the equilibrium pressure of the Cl2 gas is : 1.98 atm

Example no:14.4,Page no:623

In [6]:
#Variable declaration
Kc=10.5 
delta_n=1-3 
T=273+220 

#Calculation
Kp=Kc*(0.0821*T)**delta_n 

#Result
print"The value of the equilibrium constant of the reaction is :%.2e"%Kp

The value of the equilibrium constant of the reaction is :6.41e-03

Example no:14.6,Page no:626

In [7]:
#Variable declaration
CO2=0.236 #pressure of CO2 gas, atm
T=273+800 

#Calculation
#(a)
Kp=CO2 
#(b)
delta_n=1 
Kc=Kp*(0.0821*T)**-delta_n 

#Result
print"(a) the value of Kp of the reaction is :",Kp
print"(b) the value of Kc of the reaction is %.2e"%Kc

(a) the value of Kp of the reaction is : 0.236
(b) the value of Kc of the reaction is 2.68e-03

Example no:14.8,Page no:633

In [8]:
#Variable declaration
Kc=1.2 #equilibrium constant for the reaction
N2=.249/3.5 #conc of N2, M
H2=(3.21*10**-2)/3.5 #conc of H2, M
NH3=(6.42*10**-4)/3.5 #conc of NH3, M

#Calculation
Qc=NH3**2/(N2*H2**3) #reaction quotient initial
print"Qc=",round(Qc,3),"(approx)"

#Result
if(Qc==Kc):
    d="the system is in equilibrium" 
elif(Qc<Kc):
    d="the system is not in equilibrium and the reaction will move from left to right" 
else:
    d="the system is not in equilibrium and the reaction will move from right to left" 
print d

Qc= 0.613 (approx)
the system is not in equilibrium and the reaction will move from left to right

Example no:14.9,Page no:635

In [13]:
#Variable declaration
Kc=54.3 
H2i=0.5 #initial moles of H2
I2i=0.5 #initial moles of I2

#Calculation
#Let us assume that x moles have reacted, so, HI=2x, H2=0.5-x, I2=0.5-x, when we substitute in Kc=(HI)**2/(H2)*(I2) we get 54.3=(2x)**2/((0.5-x)*(0.5-x)) taking root we get 7.37=2*x/0.5-x
x=0.393 #from the above equation
H2=0.5-x 
I2=0.5-x 
HI=2*x 

#Result
print"The equilibrium concentration of H2 is :",H2,"M" 
print"The equilibrium concentration of I2 is :",I2,"M"
print"The equilibrium concentration of HI is :",HI,"M" 

The equilibrium concentration of H2 is : 0.107 M
The equilibrium concentration of I2 is : 0.107 M
The equilibrium concentration of HI is : 0.786 M

Example no:14.10,Page no:636

In [9]:
import math
#Variable declaration
Kc=54.3 
HIo=0.0224 
H2o=0.00623 
I2o=0.00414 
#let us assume that x moles have reacted, so, HI=HIo+2x, H2=0.00623-x, I2=0.00414-x, when we substitute in Kc=(HI)**2/(H2)*(I2) we get 54.3=(2x+0.0224)**2/((0.00623-x)*(0.00414-x)) simplifying we get 50.3x**2-0.654x+8.98*10**-4=0
a=50.3 
b=-0.654 
c=8.98*10**-4 

#Calculation
x1=(-b+math.sqrt(b**2-4*a*c))/(2*a) 
x2=(-b-math.sqrt(b**2-4*a*c))/(2*a) 
if(x1>I2o):
    x=x2 
else:
    x=x1 
H2=0.00623-x 
I2=0.00414-x 
HI=2*x+0.0224 

#Result
print"The equilibrium concentration of H2 is :",round(H2,5),"M"
print"The equilibrium concentration of I2 is :",round(I2,5),"M"
print"The equilibrium concentration of HI is :",round(HI,4),"M" 

The equilibrium concentration of H2 is : 0.00467 M
The equilibrium concentration of I2 is : 0.00258 M
The equilibrium concentration of HI is : 0.0255 M

Example no:14.11,Page no:639

In [3]:
#Variable declaration
Kc=2.37*10**-3 #equilibrium constant for the reaction
N2=0.683 #conc of N2, M
H2=8.8 #conc of H2, M
NH3=3.65 #conc of NH3, M

#Calculation
Qc=NH3**2/(N2*H2**3) #reaction quotient initial
print"Qc=%.2e"%Qc

#Result
if(Qc==Kc):
    d="the system is in equilibrium" 
elif(Qc<Kc):
    d="the system is not in equilibrium and the reaction will move from left to right" 
else:
    d="the system is not in equilibrium and the reaction will move from right to left" 
print d

Qc=2.86e-02
the system is not in equilibrium and the reaction will move from right to left