Given the three-step Solvay process for manufacturing soda ash,Na₂CO₃: CO₂(g)+ NH₃(g)+ 6 H₂O(l)→ NH₄HCO₃(aq)
NH₄HCO₃(aq)+ NaCl(aq)→ NaHCO₃(aq)+ NH₄Cl(aq)
2 NaHCO₃(aq)→ Na₂CO₃(s)+ CO₂(g)+ H₂O(l)
What mass of soda ash is produced from the reaction of 2.50 L of CO₂ at STP?

Question

Quizplus · Accepted Answer

- We have 2.50 L of CO₂ at STP.
- At STP, 1 mole of any gas occupies 22.4 L of volume.
- Therefore, 2.50 L of CO₂ is equal to 2.50/22.4 = 0.1116071 moles of CO₂.
- From the balanced chemical equation, we know that 2 moles of NaHCO₃ produce 1 mole of Na₂CO₃.
- Therefore, to calculate the mass of Na₂CO₃ produced, we need to find out how many moles of NaHCO₃ are produced first.
- From the balanced chemical equation, we know that 1 mole of CO₂ reacts with 1 mole of NH₃ and 1 mole of NaCl to produce 1 mole of NaHCO₃.
- The molar mass of CO₂ is 44.01 g/mol.
- Therefore, the mass of CO₂ used in the reaction is 44.01 x 0.1116071 = 4.919267 g.
- From the balanced chemical equation, we know that 1 mole of NH₃ reacts with 1 mole of CO₂ to produce 1 mole of NH₄HCO₃.
- Therefore, the number of moles of NH₄HCO₃ produced is also 0.1116071.
- From the balanced chemical equation, we know that 1 mole of NH₄HCO₃ reacts with 1 mole of NaCl to produce 1 mole of NaHCO₃.
- Therefore, the number of moles of NaHCO₃ produced is also 0.1116071.
- Finally, from the balanced chemical equation, we know that 2 moles of NaHCO₃ produce 1 mole of Na₂CO₃.
- Therefore, the number of moles of Na₂CO₃ produced is 0.05580355.
- The molar mass of Na₂CO₃ is 105.99 g/mol.
- Therefore, the mass of Na₂CO₃ produced is 105.99 x 0.05580355 = 5.92 g.

Given the Three-Step Solvay Process for Manufacturing Soda Ash,Na₂CO₃: CO₂(g)