Final answer:
To find how many moles of water are produced from 339 grams of SnO2, convert the mass of SnO2 to moles and then use the stoichiometry from the balanced chemical equation, resulting in 4.50 moles of H2O.
Step-by-step explanation:
The student's question involves calculating the number of moles of water (H2O) produced from a given amount of tin(IV) oxide (SnO2), based on the chemical reaction provided. To determine this, we must use stoichiometry, which is a section of chemistry that deals with the quantitative relationship between the amounts of reactants and products in a chemical reaction.
First, we convert the mass of SnO2 to moles using its molar mass. Tin(IV) oxide has a molar mass of approximately 150.71 g/mol. Dividing the given mass of SnO2 by its molar mass gives us the number of moles:
339 g SnO2 ÷ 150.71 g/mol ≈ 2.25 moles of SnO2
From the balanced chemical equation, we can see that 1 mole of SnO2 produces 2 moles of H2O. Therefore, multiplying the moles of SnO2 by this ratio gives the moles of H2O produced:
2.25 moles SnO2 × 2 moles H2O/mole SnO2 ≈ 4.50 moles of H2O