Question

For the reaction 4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6 H2O(g) ΔH∘ = −904 kJ which of the following changes will shift the equilibrium to the right, toward the formation of more products? For the reaction which of the following changes will shift the equilibrium to the right, toward the formation of more products? Increasing the volume of the reaction vessel Adding more water vapor Removing O2(g) Adding 1 atm of Ne(g) to the reaction vessel Increasing the temperature SubmitRequest Answer

Answer 1

To shift the equilibrium of the given reaction to the right, toward more product formation, the effective option is removing O2(g). Increasing the volume, adding more water vapor, adding inert Ne(g), or increasing the temperature would not shift the equilibrium to produce more products.

Step-by-step explanation:

For the reaction 4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6 H2O(g) ΔH° = −904 kJ, several factors can alter the equilibrium position:

• Increasing the volume of the reaction vessel will decrease the pressure and shift the equilibrium to the side with more gas molecules, which in this case, is the reactants side (left).
• Adding more water vapor adds a product, which shifts the equilibrium to the left, favoring reactant formation according to Le Chatelier's Principle.
• Removing O2(g) will shift the equilibrium to the right, toward the formation of more products, to compensate for the change in concentration.
• Adding 1 atm of Ne(g) to the reaction vessel will not affect the equilibrium as Ne is a noble gas and does not react with the system.
• Increasing the temperature will shift the equilibrium to favor the endothermic direction. Since the reaction is exothermic (ΔH° is negative), increasing temperature will shift the equilibrium to the left, resulting in less product formation.

Therefore, to shift the equilibrium to the right (toward product formation), removing O2(g) is the only effective option amongst those listed.

Answer 2

Increasing the volume of the reaction vessel.

Step-by-step explanation:

Let us consider the following reaction:

4 NH₃(g) + 5 O₂(g) ⇌ 4 NO(g) + 6 H₂O(g) ΔH° = −904 kJ

To assess the effect of different changes on the equilibrium we need to consider Le Chatelier Principle: if a system at equilibrium undergoes a change (in pressure, volume, etc.), it will react to counteract such change.

Increasing the volume of the reaction vessel

If volume increases, pressure decreases according to Boyle's Law. Then, the system will try to increase pressure by shifting the equilibrium towards where there are more moles of gases, that is, to the right (10 moles of gases).

Adding more water vapor

If water vapor is added, the system will try to reduce its concentration by shifting the equilibrium towards the left.

Removing O₂(g)

If oxygen is removed, the system will try to increase its concentration by shifting the equilibrium towards the left.

Adding 1 atm of Ne(g) to the reaction vessel

Adding inert gases has no effect on the equilibrium.

Increasing the temperature

This is an exothermic reaction (ΔH° < 0). If temperature is raised, the system will try to decrease it, shifting the equilibrium towards the left to absorb heat.