<P> A dry cell uses a paste electrolyte, with only enough moisture to allow current to flow . Unlike a wet cell, a dry cell can operate in any orientation without spilling, as it contains no free liquid, making it suitable for portable equipment . By comparison, the first wet cells were typically fragile glass containers with lead rods hanging from the open top and needed careful handling to avoid spillage . Lead--acid batteries did not achieve the safety and portability of the dry cell until the development of the gel battery . Wet cells have continued to be used for high - drain applications, such as starting internal combustion engines, because inhibiting the electrolyte flow tends to reduce the current capability . </P> <P> A common dry cell is the zinc - carbon cell, sometimes called the dry Leclanché cell, with a nominal voltage of 1.5 volts, the same as the alkaline cell (since both use the same zinc--manganese dioxide combination). </P> <P> A standard dry cell comprises a zinc anode, usually in the form of a cylindrical pot, with a carbon cathode in the form of a central rod . The electrolyte is ammonium chloride in the form of a paste next to the zinc anode . The remaining space between the electrolyte and carbon cathode is taken up by a second paste consisting of ammonium chloride and manganese dioxide, the latter acting as a depolariser . In some designs, the ammonium chloride is replaced by zinc chloride . </P> <P> Many experimenters tried to immobilize the electrolyte of an electrochemical cell to make it more convenient to use . The Zamboni pile of 1812 was a high - voltage dry battery but capable of delivering only minute currents . Various experiments were made with cellulose, sawdust, spun glass, asbestos fibers, and gelatine . </P>

The anode of a dry cell is made up of