In an electrolysis experiment, 0.1575 g of copper is placed on the cathode from a solution of co

step 1 Copper sulfate decomposes as CU plus 2 plus S of 4 double minus. So there are two electrons per

In an electrolysis experiment, 0.1575 g of copper is placed...

In an electrolysis experiment, $0.1575 \mathrm{g}$ of copper is placed on the cathode from a solution of copper sulfate when a current of 0.400 amperes is passed for 1200 s. $(a)$ Calculate the value of the Faraday constant. $(b)$ Given that the charge on an electron is $1.602 \times 10^{-19} \mathrm{C}$, calculate the Avogadro constant. [This experiment is described by C. A. Seiglie, $J$. Chem. Educ. 80: 668 $(2003) .]$

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Key Concepts

Elementary Charge

The elementary charge is the fundamental unit of electric charge carried by a single proton or the negative of that value for an electron. It serves as a bridge between the atomic scale of charge and the macroscopic scale, making it essential for understanding charge quantization.

Avogadro Constant

The Avogadro constant is the number of atoms, ions, or molecules in one mole of a substance. It provides a critical link between the amount of substance on a macroscopic level and the individual entities on a microscopic level, facilitating calculations that relate quantities of matter to the number of particles.

Faraday Constant

The Faraday constant is defined as the total electric charge carried by one mole of electrons. It links the microscopic transfer of electrons to the macroscopic measurement of charge in coulombs, enabling calculations that convert between the amount of substance and electrical measurements.

Electrolysis

Electrolysis is a process that uses electrical energy to drive a non-spontaneous chemical reaction. In this context, it involves the deposition of copper from a copper sulfate solution onto the cathode when an electric current is passed through the electrolyte.

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