5NaN3(s) + NaNO3(aq) → 3Na2O(s) + 8N2(g)
If 1.50 g of N2(g) are produced, how many grams of Na2O(s) are also produced?
Question 26 options:
8.85 g
3.32 g
2.05 g
2.22 g
1.24 g
To solve this problem, we need to use stoichiometry, which involves using the balanced equation to determine the mole ratios between the reactants and products.
Step 1: Find the molar mass of N2. The molar mass of N2 is 28.02 g/mol.
Step 2: Convert the given mass of N2 to moles. We are given that 1.50 g of N2 is produced, so we can calculate the moles of N2 using the equation:
moles of N2 = (mass of N2) / (molar mass of N2)
moles of N2 = 1.50 g / 28.02 g/mol
moles of N2 ≈ 0.053 mol
Step 3: Use the mole ratio from the balanced equation to determine the moles of Na2O. According to the balanced equation, the mole ratio between N2 and Na2O is 8:3. This means that for every 8 moles of N2 produced, 3 moles of Na2O are also produced.
moles of Na2O = (moles of N2) * (moles of Na2O / moles of N2)
moles of Na2O = 0.053 mol * (3/8)
moles of Na2O ≈ 0.020 mol
Step 4: Convert the moles of Na2O to grams. We can calculate the mass of Na2O using the equation:
mass of Na2O = (moles of Na2O) * (molar mass of Na2O)
mass of Na2O = 0.020 mol * (61.98 g/mol)
mass of Na2O ≈ 1.24 g
Therefore, the correct answer is 1.24 g, which is option 5.