Final answer:
The student's question about finding the mass of water produced with 25.1g of CO2 can be resolved using mole ratios and molar masses from the balanced chemical equation, with an approximate mass of 10.27g calculated for water.Answer is OPTION A
Step-by-step explanation:
To determine the mass of water produced along with 25.1g of carbon dioxide, we can use stoichiometry from the balanced chemical equation. The equation for the combustion of a hydrocarbon, like glucose, is typically represented as:
C6H12O6 + 6O2 -> 6CO2 + 6H2O
From this equation, we can see the mole ratio of carbon dioxide to water is 1:1. Now, to find the mass of water produced, we'll utilize the molar masses of CO2 and H2O.
The molar mass of CO2 is approximately 44.01 g/mol, and the molar mass of water (H2O) is approximately 18.015 g/mol. Given that 25.1 g of CO2 is produced, let's first find out how many moles of CO2 this represents:
- 25.1 g CO2 * (1 mol CO2 / 44.01 g CO2) = 0.570 moles of CO2
- The same number of moles of water will be produced since the ratio is 1:1.
- Now, we'll convert the moles of water to grams: 0.570 moles of H2O * (18.015 g H2O / 1 mol H2O) = 10.27 g of H2O.
Therefore, the mass of water produced is closest to option a. 9.0g, but since this is not the exact answer, we should review the question to make sure no alternatives or ranges are given and then choose the best fit.