Bromine dichloride, BrCl2, decomposes to form bromine and chlorine at equilibrium according to the following equation:

2BrCl2 (g) + heat ⇌ Br2 (g) + 2Cl2 (g)

For the following change, how would the reaction shift (toward the products, reactants, or no change) ?

The temperature is increased?

Question

Kaiden

Chemistry

23 May, 17:33

Bromine dichloride, BrCl2, decomposes to form bromine and chlorine at equilibrium according to the following equation:

2BrCl2 (g) + heat ⇌ Br2 (g) + 2Cl2 (g)

For the following change, how would the reaction shift (toward the products, reactants, or no change) ?

The temperature is increased?

+3

Answers (1)

Know the Answer?

Mohammad Henderson · Answer 1

Heat is a reactant in this equilibrium and increasing temperature is another way to say adding heat. So, how does the reaction shift when you add a reactant?

Bromine dichloride, BrCl2, decomposes to form bromine and chlorine at equilibrium according to the following equation:2BrCl2 (g) + heat ⇌ Br2 (g) + 2Cl2 (g)For the following change, how would the reaction shift (toward the products, reactants, or no change) ?The temperature is increased?

Bromine dichloride, BrCl2, decomposes to form bromine and chlorine at equilibrium according to the following equation:

2BrCl2 (g) + heat ⇌ Br2 (g) + 2Cl2 (g)

For the following change, how would the reaction shift (toward the products, reactants, or no change) ?

The temperature is increased?