Question

How many grams of na2co3 would be needed to produce 1000g of nahco3

Answer 1

630.95 grams of Na₂CO₃ would be needed to produce 1000g of NaHCO₃

Step-by-step explanation:

The balanced reaction is:

Na₂CO₃ + CO₂+ H₂O → 2 NaHCO₃

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:

• Na₂CO₃: 1 moles
• CO₂: 1 mole
• H₂O: 1 mole
• NaHCO₃: 2 moles

Being the molar mass:

• Na₂CO₃: 106 g/mole
• CO₂: 44 g/mole
• H₂O: 18 g/mole
• NaHCO₃: 84 g/mole

Then by stoichiometry the following quantities of mass participate in the reaction:

• Na₂CO₃: 1 mole* 106 g/mole= 106 g
• CO₂: 1 mole* 44 g/mole= 44 g
• H₂O: 1 mole* 18 g/mole= 18 g
• NaHCO₃: 2 moles* 84 g/mole= 168 g

You can apply the following rule of three: if 106 grams of Na₂CO₃ are needed to produce 168 grams of NaHCO₃, how much mass of Na₂CO₃ is necessary to produce 1000 grams of NaHCO₃?

`mass of Na_(2) CO_(3)=(1000grams ofNaHCO_(3) *106gramsofNa_(2) CO_(3) )/(168grams ofNaHCO_(3))`

mass of Na₂CO₃= 630.95 grams

630.95 grams of Na₂CO₃ would be needed to produce 1000g of NaHCO₃