Final answer:
To find out how many grams of NO are produced from 15.8 g of H2O, we first convert the mass of H2O to moles, then use the molar ratio from the balanced chemical equation to find the moles of NO produced, and finally convert these moles to grams, yielding 17.52 grams of NO.
Step-by-step explanation:
To determine how many grams of NO are produced from 15.8 g of H2O, we need to use stoichiometry and the balanced chemical equation for the reaction. Unfortunately, the reaction in question is not provided, but assuming it involves the production of NO from H2O, a common industrial process can be used for illustration. If the balanced equation is 4NO(g) + 6H2O(g) → something else, we can establish the molar relationship between NO and H2O.
First, we calculate the number of moles of H2O using its molar mass (18.02 g/mol):
moles H2O = 15.8 g H2O × (1 mol H2O / 18.02 g H2O) = 0.877 moles H2O
According to the hypothetical reaction, the molar ratio of NO to H2O is 4:6, which simplifies to 2:3. Therefore, the number of moles of NO produced would be:
moles NO = 0.877 moles H2O × (2 moles NO / 3 moles H2O) = 0.584 moles NO
Finally, we convert the moles of NO to grams using the molar mass of NO (30.00 g/mol):
grams NO = 0.584 moles NO × 30 g/mol = 17.52 grams NO