Consider the reaction 2 Br(g) <=> Br2(g), which is exothermic as written. What w

Question

Consider the reaction 2 Br(g) <=> Br2(g), which is exothermic as written. What would be the effect on the equilibrium position of removing Br(g)?

1. Reaction would go to the right, making more "products"

2. No change on the equilibrium position

3. Reaction would go to the left, making more "products"

4. Reaction would go to the right, making more "reactants"

5. Reaction would go to the left, making more "reactants" 1 points Saved

QUESTION 12 Consider the reaction 2 Cl(g) <=> Cl2(g), which is exothermic as written. What would be the effect on the equilibrium position of increasing the volume of the reaction container?

1. Reaction would go to the left, making more "reactants"

2. Reaction would go to the right, making more "products"

3. No change on the equilibrium position

4. Reaction would go to the right, making more "reactants"

5. Reaction would go to the left, making more "products"

Explanation / Answer

1.

If Br is removed from the reaction, there is decrease of reactant concentration. So the equilibrium will shift to left making more reactants until getting the equilibrium

2.

If volume is decreased, according to Lechatlier's principle the equilibrium will shifts in a direction where there are more number of moles

So in the reaction if volume is increasing, the equilibrium will shifts from right to left making more reactants

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.