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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
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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?

User Mduvall
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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?
User Skuntsel
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