Final answer:
To find the mass of SnO2 that reacts with 12.00 grams of hydrogen, we first determine the number of moles of hydrogen and then use the ratio from the balanced equation to calculate the moles of SnO2 required, which are then converted to grams using the molar mass of SnO2.
Step-by-step explanation:
The student asked how many grams of SnO2 react with 12.00 grams of hydrogen using the the chemical equation SnO2(s) + 2H2(g) → 2H2O(l) + Sn(s). To answer this question, we need to use molar stoichiometry and the balanced equation provided to find the relationship between the mass of hydrogen and SnO2.
First, we should calculate the molar mass of H2, which is 2.02 g/mol, and find out how many moles 12.00 grams of hydrogen represent. With 12.00 grams of H2, we have 12.00 g / 2.02 g/mol = 5.94 moles of H2. According to the balanced equation, 2 moles of H2 react with 1 mole of SnO2. Therefore, 5.94 moles of H2 would react with 5.94 / 2 = 2.97 moles of SnO2.
Now, we need to find the molar mass of SnO2. Sn has a molar mass of about 118.71 g/mol and O has a molar mass of about 16.00 g/mol. So, one mole of SnO2 would have a molar mass of 118.71 g (for Sn) + 2 * 16.00 g (for O) = 150.71 g/mol. Therefore, the mass of SnO2 needed would be 2.97 moles * 150.71 g/mol = 447.6097 grams. However, options provided are not close to this value, which suggests there might be a typo in the question's options.