Aqueous calcium bromide was mixed with aqueous gold(I) perchlorate, and a crystallized gold(I) bromide product was formed. Consider the other product and its phase, and then write the balanced molecular equation for this precipitation reaction.

CaBr2(aq)+2AuClO4(aq)�¨2AuBr(s)+Ca(ClO4)2(aq)

Cl(Clo4)

To determine the balanced molecular equation for the precipitation reaction, we need to identify the other product formed when aqueous calcium bromide reacts with aqueous gold(I) perchlorate.

We know that the reaction between a bromide compound and a perchlorate compound typically leads to the exchange of the anions, resulting in the formation of a new bromide compound and a new perchlorate compound.

Given that aqueous gold(I) perchlorate is the reactant, it will react with the aqueous calcium bromide to form a gold(I) bromide compound and a new perchlorate compound. Since calcium is more reactive than gold, it will displace gold from the perchlorate, leading to the formation of calcium perchlorate.

Now, let's write the balanced molecular equation for this precipitation reaction:

CaBr2 (aq) + AuClO4 (aq) → AuBr (s) + Ca(ClO4)2 (aq)

In this equation, the reactants are aqueous calcium bromide (CaBr2) and aqueous gold(I) perchlorate (AuClO4). The products are solid gold(I) bromide (AuBr) and aqueous calcium perchlorate (Ca(ClO4)2).

Therefore, the balanced molecular equation for this precipitation reaction is:

CaBr2 (aq) + AuClO4 (aq) → AuBr (s) + Ca(ClO4)2 (aq)

CaBr(aq) + AuClO4(aq) ==> AuBr(s) + ??

This appears to be a double replacement reaction. Can you fill in the missing material?