Consider the following equilibrium between oxides of nitrogen: 3NO (g) --><-- NO

Question

Consider the following equilibrium between oxides of nitrogen:

3NO (g) --><-- NO2(g) + N2O(g) delta H=-155.7 kJ

How will each of the following changes affect the amount of NO2 at equilibrium? How will it affect K?

Change

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

Change

NO2 K NO is added

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

The temperature is decreased

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

The volume is halved

Increase?

Decrease?

Nothing?

Increase?

Decrease?

Nothing?

Explanation / Answer

1)we are adding a reactant

According to LeChattelier's Principle,

Adding reactant will shift reaction towards product side

Equilibrium moves to product side

NO2 increases

K will be constant as Temperature is constant

2)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

Equilibrium moves to product side

NO2 increases

K increases

3)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

Equilibrium moves to product side

NO2 increases

K will be constant as Temperature is constant

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