contestada

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

Respuesta :

Willchemistry

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.

mahima6824soni

The effect on the equilibrium position of increasing the temperature is  the Reaction would go to the right, making more "products"

What is an endothermic reaction?

In the endothermic reaction, there is an increase in the enthalpy in the system.

Examples are evaporation, melting, boiling.

Given reaction is

[tex]\bold{Cl_2(g) + Br_2(g) <=> 2 BrCl(g)}[/tex]

This is an endothermic reaction, and it is a reversible reaction, as it is taking energy to break the bonds.

Thus, the correct option is 1.

Learn more about endothermic reactions, here:

https://brainly.com/question/2192784

Otras preguntas