When 10.0 g of glucose (C6H12O6) is completely combusted in excess oxygen, what is the total combined mass of carbon dioxide (CO2) and water (H2O) produced?

• A. 10.0 g + mass of oxygen consumed
• B. 10.8 g
• C. 10.0 g
• D. 14.7 g

Answer: (A)

Verified step by step guidance

1. Write the balanced chemical equation for the complete combustion of glucose (C6H12O6): \[ \mathrm{C_6H_{12}O_6 + 6O_2 \rightarrow 6CO_2 + 6H_2O} \]
2. Calculate the molar mass of glucose (C6H12O6) by summing the atomic masses: \[ M_{C_6H_{12}O_6} = 6 \times M_C + 12 \times M_H + 6 \times M_O \]
3. Determine the number of moles of glucose combusted using the given mass: \[ n = \frac{\text{mass of glucose}}{M_{C_6H_{12}O_6}} \]
4. Use the stoichiometry from the balanced equation to find the moles of CO2 and H2O produced: - Moles of CO2 = 6 \times n - Moles of H2O = 6 \times n
5. Calculate the total mass of CO2 and H2O produced by multiplying their moles by their respective molar masses and summing: \[ \text{mass}_{CO_2} = n_{CO_2} \times M_{CO_2} \] \[ \text{mass}_{H_2O} = n_{H_2O} \times M_{H_2O} \] \[ \text{total mass} = \text{mass}_{CO_2} + \text{mass}_{H_2O} \]