When 25.5 grams of NaHCO3 decompose completely, what mass of CO2 is produced? (Molar masses: NaHCO3 = 84.0 g/mol, CO2 = 44.0 g/mol)

• A. 44.0 grams
• B. 13.4 grams
• C. 25.5 grams
• D. 6.7 grams

Answer: (B)

Verified step by step guidance

1. Write the balanced chemical equation for the decomposition of sodium bicarbonate (NaHCO\_3): \[\mathrm{2\ NaHCO\_3 \rightarrow Na\_2CO\_3 + CO\_2 + H\_2O}\]
2. Calculate the number of moles of NaHCO\_3 decomposed using its molar mass: \[\text{moles of NaHCO\_3} = \frac{\text{mass of NaHCO\_3}}{\text{molar mass of NaHCO\_3}} = \frac{25.5\ \mathrm{g}}{84.0\ \mathrm{g/mol}}\]
3. Use the mole ratio from the balanced equation to find the moles of CO\_2 produced. According to the equation, 2 moles of NaHCO\_3 produce 1 mole of CO\_2, so: \[\text{moles of CO\_2} = \frac{1}{2} \times \text{moles of NaHCO\_3}\]
4. Calculate the mass of CO\_2 produced by multiplying the moles of CO\_2 by its molar mass: \[\text{mass of CO\_2} = \text{moles of CO\_2} \times 44.0\ \mathrm{g/mol}\]
5. This final value will give you the mass of CO\_2 produced from the complete decomposition of 25.5 grams of NaHCO\_3.