During the vital first synthesis step for preparing potassium dichromate, moles of solid chromite ore () are forcefully roasted with sodium carbonate () and atmospheric oxygen (). According to the str

Question

During the vital first synthesis step for preparing potassium dichromate, $4$ moles of solid chromite ore ($FeCr_2O_4$) are forcefully roasted with sodium carbonate ($Na_2CO_3$) and atmospheric oxygen ($O_2$). According to the strictly balanced stoichiometric equation for this specific step, exactly how many moles of $CO_2$ gas are liberated?

Prashant Kotian · Accepted Answer

Correct answer: 8. The balanced chemical equation for the oxidative roasting of chromite ore is: . The stoichiometry rigidly dictates that for every moles of the reactant consumed, precisely moles of are produced and vented.

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