Question

In the Haber process shown below, predict the direction in which this exothermic reaction will shift when the system conditions are changed as follows: N2(g) + 3 H2(g)  2 NH3(g)

A. The amount of N2(g) is increased Left No Change Right

B. The amount of NH3(g) is decreased Left No Change Right

C. The temperature is increased Left No Change Right

D. The pressure is reduced Left No Change Right

E. A catalyst is added Left No Change Right

Answer 1

A)

we are adding a reactant

According to Le Chatelier's Principle,

Adding reactant will shift reaction towards product side

Answer: Right

B)

we are removing a product

According to Le Chatelier's Principle,

Removing product will shift reaction towards product side

Answer: right

C)

Forward reaction is exothermic in nature

we are increasing temperature or adding heat here

so, according to Le Chatelier's principle,

equilibrium will move in direction which absorbs heat

hence, backward reaction will be favoured

Answer: left

D)

We are decreasing pressure here

so, according to Le Chatelier'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: left

E)

Catalyst doesn't affect equilibrium

Answer: No change