Explain the differences between a primary galvanic cell-one that is not rechargeable- and a storage cell (for example, the lead storage battery), which is rechargeable.

A primary galvanic cell, often referred to simply as a primary cell, is a battery that is designed to be used once and then disposed of. The primary galvanic cell achieves the conversion of chemical energy to electrical energy through a chemical reaction that is irreversible. Inside these cells, you'll find two dissimilar metals or metal compounds known as the cathode and anode, submerged in an electrolyte solution. As they function, one metal is oxidized (loses electrons), while the other is reduced (gains electrons), thus producing an electric current.

Let’s take the classic example of a zinc-carbon cell: zinc serves as the anode, while manganese dioxide acts as the cathode, and the electrolyte is often a paste of ammonium chloride. When the cell is in use, zinc gets oxidized, and the manganese dioxide is reduced, resulting in the flow of electrons from the anode to the cathode. Once the reactants are depleted, the cell can no longer produce electricity and is 'dead'.

In contrast to primary cells, rechargeable batteries, or secondary cells, have the ability to be recharged and reused multiple times. This is possible because the chemical reactions that occur during discharge are generally reversible. By applying an external electric current, the discharge process is reversed, thus reinvigorating the battery's capacity to provide electrical power.

These batteries are widely utilized in various applications including mobile phones, laptops, and electric vehicles. They offer greater convenience and environmental benefits by reducing waste. The efficiency and lifespan of these batteries can vary based on the technology and materials used, as well as how they are maintained. Some common types of rechargeable batteries include lithium-ion, nickel-cadmium (NiCd), and nickel-metal hydride (NiMH).

One specific type of rechargeable battery is the lead-acid battery, which is well-known for its use in vehicles. It comprises of lead dioxide as the positive plate, sponge lead as the negative plate, and a sulfuric acid solution as the electrolyte. The way it works is fascinating: during discharge, the lead dioxide (PbO₂) and the sponge lead (Pb) transform into lead sulfate (PbSO₄) while the sulfuric acid becomes water, thereby releasing electrical energy. When you charge the battery, the process is reversed, and lead dioxide and sponge lead are recreated.

In fact, the lead-acid battery is lauded for its high surge currents, meaning it's great for applications where a large current is needed for a short period, like starting a car's engine. Plus, they are cost-effective and have a reliable track record, though they are heavier and have a lower energy density compared to newer battery technologies.

The conversion of chemical energy to electrical energy is a marvel of modern technology that is essential to many of the devices we use every day. This conversion is primarily facilitated by an electrochemical reaction wherein the difference in energy between reactants and products is harnessed and converted into a flow of electrons, or electricity.

For primary and rechargeable batteries alike, as the reaction proceeds, electrons are compelled to move from the anode to the cathode, creating a current. This flow can then be directed to power electronic devices. The efficiency of this conversion process is critical: it determines how much power a battery can deliver and how long it will last before needing to be recharged or replaced. Innovations continue to be made in this field to develop more efficient energy conversion methods, to maximize energy storage, and to minimize environmental impact.