Refer to the (unbalanced) equation CS₂ + CaO $\rarr$ CO₂ + CaS. How many grams of CaS are produced if 53 g of CO₂ are produced

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Quizplus · Accepted Answer

The unbalanced equation is CS₂ + CaO F1F1F1S1F1F1F10 CO₂ + CaS. For every 1 mole of CS₂ reacted, 1 mole of CaS is produced. Molar mass of CO₂ = 60.07 g/mol Number of moles of CO₂ = 53 g / 60.07 g/mol = 0.8828 mol Therefore, 0.8828 mol of CaS is produced. Molar mass of CaS = 72.15 g/mol Mass of CaS produced = 0.8828 mol x 72.15 g/mol = 63.27 g ≈ 170 g.

Refer to the (Unbalanced) Equation CS2 + CaO →\rarr→ CO2 + CaS

Refer to the (Unbalanced) Equation CS₂ + CaO $\rarr$ CO₂ + CaS