Consider the reaction Cl 2 (g) + Br 2 (g) 2 BrCl (g), which is endothermic as written. What would be the effect on the equilibrium position of increasing the temperature? 1. Reaction would go to the right, making more "products" 2. Reaction would go to the left, making more "products" 3. Reaction would go to the left, making more "reactants" 4. Reaction would go to the right, making more "reactants" 5. No change on the equilibrium position

Question

Walker Castaneda

Chemistry

11 September, 06:33

Consider the reaction Cl 2 (g) + Br 2 (g) 2 BrCl (g), which is endothermic as written. What would be the effect on the equilibrium position of increasing the temperature? 1. Reaction would go to the right, making more "products" 2. Reaction would go to the left, making more "products" 3. Reaction would go to the left, making more "reactants" 4. Reaction would go to the right, making more "reactants" 5. No change on the equilibrium position

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Answers (2)

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Benjamin Barton · Answer 1

According to Le Châtelier's principle, an increase in temperature favors the endothermic process. Since the reaction, which proceeds towards bromine chloride, is endothermic, the reaction would shift right, making more products.

Johnathon Hunter · Answer 2

Hey there!:

endothermic reaction can be represented by:

A + heat B

So when temperature is decreased, the system tries to oppose the change. SO it moves to the side where the temperature increases. I f it moves to product side, the temperature decreases as it it absorbing heat to form products.

So the system moves to the reactants side.