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Four moles of lithium react per mole of iron disulfide. Using molar masses $M_{\mathrm{Li}}=6.94\mathrm{g}\mathrm{mo}{\mathrm{l}}^{-1}$, $M_{\mathrm{Fe}}=55.845\mathrm{g}\mathrm{mo}{\mathrm{l}}^{-1}$ and $M_{\mathrm{S}}=32.06\mathrm{g}\mathrm{mo}{\mathrm{l}}^{-1}$ givesThus the stoichiometric mass ratio is Li:FeS₂ = 1:4.322, or approximately 18.79 wt% lithium and 81.21 wt% iron disulfide within the combined active reactants. This excludes electrolyte, current collectors, casing and any deliberate excess of one reactant. The underlying conversion reaction, rather than the nominal cell voltage, sets that ratio.^[ref]

This lithium iron disulfide battery consumes a metallic lithium anode and converts iron disulfide into iron and lithium sulfide. Commercial cells of this chemistry are primary batteries. A conventional lithium-ion battery is designed for reversible cycling: lithium ions transfer between two host electrodes, commonly a carbon insertion anode and a transition-metal compound cathode, while electrons travel in the external circuit. Metallic lithium is not the intended normal anode reactant in that design. Primary Li/FeS₂ conversion is the key distinction from the rechargeable lithium-ion host-electrode system. The fact that both transport lithium ions does not make them the same battery chemistry, and a nominal 1.5 V is not a definition of either class.^[ref]