For the reaction, calculate how many grams of the product form when 3.2 g of Na2O completely reacts.
Assume that there is more than enough of the other reactant.
Na2O(s)+H2O(l)→2NaOH(aq)
mols Na2O = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Na2O to mols NaOH. That will be mols NaOH = 2 x mols Na2O
Now convert mols NaOH to grams NaOH. grams = mols x molar mass
To solve this problem, we need to use stoichiometry to calculate the number of grams of the product formed when a given amount of reactant is consumed.
Step 1: Write and balance the chemical equation:
Na2O(s) + H2O(l) → 2NaOH(aq)
Step 2: Calculate the molar mass of Na2O:
Na2O: (2 * atomic mass of Na) + atomic mass of O = (2 * 22.99 g/mol) + 16.00 g/mol = 61.98 g/mol
Step 3: Determine the number of moles of Na2O:
moles of Na2O = mass of Na2O / molar mass of Na2O = 3.2 g / 61.98 g/mol = 0.052 moles
Step 4: Use the stoichiometric ratio from the balanced equation to find the number of moles of NaOH produced:
From the balanced equation, we can see that 1 mole of Na2O produces 2 moles of NaOH.
moles of NaOH = 0.052 moles Na2O * (2 moles NaOH / 1 mole Na2O) = 0.104 moles
Step 5: Convert moles of NaOH to grams:
To convert moles of NaOH to grams, we need to multiply by the molar mass of NaOH.
molar mass of NaOH: (atomic mass of Na) + (atomic mass of O) + (atomic mass of H) = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 40.00 g/mol
grams of NaOH = moles of NaOH * molar mass of NaOH = 0.104 moles * 40.00 g/mol = 4.16 grams
Therefore, when 3.2 grams of Na2O completely reacts, 4.16 grams of NaOH will be produced.