Question

If you had a sample of 10.0g of pure NaHCO and heated it until it had completely decomposed how much mass would be lost.

Answer 1

The mass lost during the complete decomposition of 10.0g of pure NaHCO₃ would be approximately 2.2g.

Step-by-step explanation:

When sodium bicarbonate (NaHCO₃) is heated, it undergoes a chemical decomposition, releasing carbon dioxide (CO₂), water (H₂O), and leaving behind a residue of sodium carbonate (Na₂CO₃). The chemical equation for this reaction is:

`\[2NaHCO₃ \rightarrow \text{Heat} \rightarrow Na₂CO₃ + H₂O + CO₂.\]`

The molar mass of NaHCO₃ is approximately 84 grams/mol. This means that in 10.0g of NaHCO₃, there are
`\( \frac{10.0 \, \text{g}}{84 \, \text{g/mol}} \approx 0.119 \, \text{mol} \) of NaHCO₃.`

According to the balanced equation, two moles of NaHCO₃ produce one mole of CO₂. Therefore, the moles of CO₂ produced in the reaction would be
`\(0.119 \, \text{mol} * \frac{1 \, \text{mol CO₂}}{2 \, \text{mol NaHCO₃}} = 0.0595 \, \text{mol CO₂}.\)`

The molar mass of CO₂ is approximately 44 grams/mol. Hence, the mass of CO₂ produced would be
`\(0.0595 \, \text{mol} * 44 \, \text{g/mol} = 2.618 \, \text{g}.\)`

Therefore, the mass lost during the complete decomposition of 10.0g of pure NaHCO₃ is the mass of CO₂ produced, which is approximately
`\(2.618 \, \text{g}.\)`