The Haber process system is shown below: N 2 (g) + 3H 2 (g) 2NH 3 (g) K c = 1.2

Question

The Haber process system is shown below:

N2 (g) + 3H2 (g) 2NH3 (g) Kc= 1.2 (at 375°C); H° = -92 kJ

Assuming the system is at equilibrium, please answer one of (l --> r), (r -->l), or (no shift) to the following possible pertubations:

a. Some N2 (g) is added _______

b. Some H2 (g) is added _______

c. Some NH3 (g) is added ________

d. Some NH3 (g) is removed _______

e. The temperature is lowered _______

f. The volume is decreased ________

g. The pressure is decreased _______

h. A fresh batch of catalyst is added ______

Please calculate the value of Kp at 375°C.

Explanation / Answer

1)

a)we are adding a reactant

According to LeChattelier's Principle,

Adding reactant will shift reaction towards product side

Answer: l —> r

b)we are adding a reactant

According to LeChattelier's Principle,

Adding reactant will shift reaction towards product side

Answer: l —> r

c)we are adding a product

According to LeChattelier's Principle,

Adding product will shift reaction towards reactant side

Answer: r —> l

d)we are removing a product

According to LeChattelier's Principle,

Removing product will shift reaction towards product side

Answer: l —> r

e)Forward reaction is exothermic in nature

we are decreasing temperature or removing heat here

so, according to Le Chatellier's principle,

equilibrium will move in direction which release heat

hence, forward reaction will be favoured

Answer: l —> r

f)We are decreasing volume here

In other words we are trying to increase pressure

so, according to Le Chatellier's principle,

Reaction will try to decrease the pressure

Hence it will move in a direction which have lesser gaseous molecules

Here product has less gaseous molecule

So equilibrium will move to right

Answer: l —> r

g)We are decreasing pressure here

so, according to Le Chatellier's principle,

Reaction will try to increase the pressure

Hence it will move in a direction which have more gaseous molecules

Here reactant has more gaseous molecule

So equilibrium will move to left

Answer: r —> l

h)Catalyst doesn't affect equilibrium

Answer: No eshift

2)

T = 375.0 oC =(375.0 + 273) K= 648.0 K

delta n = number of gaseous molecule in product - number of gaseous molecule in reactant

delta n = -2

Kp= Kc (RT)^delta n

Kp = 1.2*(0.0821*648.0)^(-2)

Kp = 0.000424

Answer: 4.24*10^-4

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