Final answer:
Zinc (Zn) in the reaction acts as a reducing agent. To find the number of molecules and mass of Zn(CN)₂ produced from 35.27 g of K[Ag(CN)₂], we need to calculate the moles using the molar mass of reactants and products, then apply Avogadro's number and the molar mass of Zn(CN)₂, respectively.
Step-by-step explanation:
In the chemical reaction 2K[Ag(CN)₂] + Zn(s) → 2Ag(s) + Zn(CN)₂ + 2KCN, zinc (Zn) serves as a reducing agent. It donates electrons to the other reactants, in this case, to the Ag(CN)₂ complex, which allows the silver ions to gain electrons and be recovered as solid silver.
In terms of the reaction, when 35.27 g of K[Ag(CN)₂] reacts, it will produce a stoichiometrically equivalent quantity of Zn(CN)₂ based on the molar mass of K[Ag(CN)₂] and Zn(CN)₂.
To calculate the number of molecules of Zn(CN)₂ produced, we would first need to calculate the number of moles of K[Ag(CN)₂] present in 35.27 g, and then use Avogadro's number to convert moles to molecules.
For calculating the mass of Zn(CN)₂ produced, the number of moles of Zn(CN)₂, which will be the same as the moles of K[Ag(CN)₂] used, will then be multiplied by the molar mass of Zn(CN)₂ to determine the mass.