Consider this reaction at equilibrium: 2H₂O₂(g) 2H₂O(g) + O₂(g) , ΔHº_rxn = -210 kJ/mol
If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?

Question

Consider this reaction at equilibrium: 2H₂O₂(g)

Consider this reaction at equilibrium: 2H<sub>2</sub>O<sub>2</sub>(g) 2H<sub>2</sub>O(g) + O<sub>2</sub>(g) , ΔHº<sub>rxn</sub> = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium? A) A shift to produce more H<sub>2</sub>O<sub>2</sub> B) A shift to produce more O<sub>2</sub> C) No change will occur. D) A shift to produce less H<sub>2</sub>O E) The pressure decreases.

2H₂O(g) + O₂(g) , ΔHº_rxn = -210 kJ/mol
If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?

Quizplus · Accepted Answer

The Answer of Consider this reaction at equilibrium: 2H₂O₂(g) 2H₂O(g) + O₂(g), ΔHº_rxn = -210 kJ/mol If the volume of the system is expanded at constant temperature, what change will occur in the position of the equilibrium?

Consider This Reaction at Equilibrium: 2H2O2(g) 2H2O(g) + O2(g)

Consider This Reaction at Equilibrium: 2H₂O₂(g) 2H₂O(g) + O₂(g)