When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 19.2 g of carbon were burned in the presence of 61.2 g of oxygen, 10.0 g of oxygen remained unreacted. What mass of carbon dioxide was produced

We will produce 70.4 grams of CO2

Explanation:

Step 1: Data given

Mass of carbon = 19.2 grams

Mass of oxygen = 61.2 grams

Mass of oxygen remaining = 10.0 grams

Molar mass carbon = 12.01 g/mol

Molar mass Oxygen = 32.0 g/mol

Step 2: The balanced equation

C + O2 → CO2

Step 3: Calculate moles

Moles = mass / molar mass

Moles Carbon = 19.2 grams / 12.01 g/mol = 1.60 moles

For 1 mol carbon we need 1 mol oxygen to produce 1 mol carbon dioxide

For 1.6 moles carbon we have 1.6 moles oxygen

Step 4: Calculate mass oxygen reacted

Mass oxygen = 1.6 moles * 32.0 g/mol

Mass oxygen = 51.2 grams oxygen reacted

Remaining mass oxygen = 61.2 grams - 51.2 grams = 10.0 grams

Step 5: Calculate moles CO2

For 1 mol carbon we need 1 mol oxygen to produce 1 mol carbon dioxide

For 1.6 moles carbon we'll have 1.6 moles CO2

Step 6: Calculate mass CO2

Mass CO2 = moles * molar mass

Mass CO2 = 1.6 moles * 44.01 g/mol

Mass CO2 = 70.4 grams

We will produce 70.4 grams of CO2

O2 = 1.6 moles