Question

How will this system at equilibrium be affected by each of the conditions stated here? 2 Upper H Subscript 2 Baseline (g) Upper O Subscript 2 Baseline (g) double-headed arrow 2 Upper H Subscript 2 Baseline Upper O (g) heat. Removal of H2O addition of O2 decrease in pressure increase in temperature.

Answer 1

In a reversible reaction the conditions of the reaction determines the direction to which the equilibrium position will shift.

The equation of the reaction is;

2H2(g) + O2(g) + ⇄ 2H2O(g) + Heat

• We can see that the reaction is exothermic since heat is a product in the reaction. Hence an increase in temperature will favor the reverse reaction.

• Removal of water from the system will shift the equilibrium position to the right encouraging more products to be formed.

• Addition of more O2 to the system will favor the forward reaction causing more H2O to be formed.

Learn more about reaction equilibrium:brainly.com/question/11114490