Write a balanced chemical equation based on the following description:
aqueous iridium(III) bromide reacts with aqueous silver acetate to form
solid silver bromide and aqueous iridium(III) acetate

IrBr₃(aq) + 3AgC₂H₃O₂(aq) ⟶ Ir(C₂H₃O₂)₃(aq) + 3AgBr(s)  

Explanation:

Iridium(III) bromide(aq) + silver acetate(aq) ⟶ iridium(III) acetate + silver bromide

You have probably learned NAG SAG and "Cats Cradle Old People," Sally Said.

I've listed the rules below.

The PMS group are the exception to the rule that halides are usually soluble.

We can use the solubility rules to decide which product is the precipitate.

Iridium(III) acetate — soluble (Acetate)

Silver bromide — insoluble (PMS,  Silver halide)

So silver bromide is a precipitate.

The word equation becomes

Iridium(III) bromide(aq) + silver acetate(aq) ⟶ iridium(III) acetate(aq) + silver bromide(s)

In symbols, the equation is

IrBr₃(aq) + 3AgC₂H₃O₂(aq) ⟶ Ir(C₂H₃O₂)₃(aq) + 3AgBr(s)

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24