The reaction for the synthesis of ammonia N2(g) + 3 H2(g) → 2 NH3(g) is exothermic. Increasing the temperature applied to the system I) increases the amount of NH3. II) decreases the amount of NH3. III) changes the value of Keq. IV) does not change the value of Keq.

The correct statements are (II) and (III).

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

This is a type of exothermic reaction because heat is released in the reaction.

On increasing the temperature

If the temperature is increased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where decrease in temperature occurs. As, this is an exothermic reaction, forward reaction will increase the temperature. Hence, the equilibrium will shift in the left direction.

And by moving to left side amount of ammonia will decrease accompanied by the change in the value of an equilibrium constant.

there all right good

explanation:

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.