Predict whether the equilibria
I) CO2(g) + 2 NH3(g) =
CO(NH2)2(s) + H2O(g),
AH° = -90 kJ
II) Ni(s) + 4 CO(g) = Ni(CO)4(8),
AH° = -161 kJ
will shift toward products or reactants with a
temperature increase.
1. I shifts toward reactants and II shifts
toward products.
2. Both I and II shift toward products.
3. Unable to determine
4. Both I and II shift toward reactants.
5. I shifts toward products and II shifts to-
ward reactants.

The correct answer is option 4.

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 exothermic reaction :ΔH = negative

For the given equation:

I) ,ΔH° = -90 kJ

On Increasing the temperature

This is an exothermic reaction, backward reaction will decrease the temperature. Hence, the equilibrium will shift in the left direction that is towards reactants.

II) ,ΔH° = -161 kJ

On Increasing the temperature

This is an exothermic reaction, backward reaction will decrease the temperature. Hence, the equilibrium will shift in the left direction that is towards reactants.

b.

the accuracy of the data.