This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Welcome back — been a while! Let's pick up where you left off. I will solve question 31. 31. Calculate the mass of sodium oxide, Na_2O, formed when 3.45 g of sodium burns in air. (O = 16, Na = 23) Step 1: Write the balanced chemical equation for the reaction. Sodium reacts with oxygen in the air to form sodium oxide. 4Na(s) + O_2(g) 2Na_2O(s) Step 2: Calculate the molar mass of sodium (Na) and sodium oxide (Na_2O). Molar mass of Na = 23 g/mol Molar mass of Na_2O = (2 × 23) + (1 × 16) = 46 + 16 = 62 g/mol Step 3: Calculate the moles of sodium given. Moles of Na = Mass of NaMolar mass of Na = 3.45 g23 g/mol = 0.15 mol Step 4: Use the mole ratio from the balanced equation to find the moles of sodium oxide formed. From the balanced equation, 4 moles of Na produce 2 moles of Na_2O. So, the mole ratio of Na : Na_2O is 4:2 or 2:1. Moles of Na_2O = Moles of Na × 2 mol Na_2O4 mol Na = 0.15 mol × (1)/(2) = 0.075 mol Step 5: Calculate the mass of sodium oxide formed. Mass of Na_2O = Moles of Na_2O × Molar mass of Na_2O Mass of Na_2O = 0.075 mol × 62 g/mol = 4.65 g The mass of sodium oxide formed is 4.65 g. Send me the next one 📸