Question

Liquid hexane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 4.3 g of hexane is mixed with 7.14 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to significant digits.

Answer 1

We can produce 6.20 grams of CO2

Step-by-step explanation:

Step 1: Data given

Mass of hexane = 4.3 grams

Molar mass of hexane = 86.18 g/mol

Mass of oxygen = 7.14 grams

Molar mass of oxygen = 32.0 g/mol

Step 2: The balanced equation

2C6H14 + 19O2 → 12CO2 + 14H2O

Step 3: Calculate moles

Moles = mass / molar mass

Moles hexane = 4.3 grams / 86.18 g/mol

Moles hexane = 0.0499 moles

Moles oxygen = 7.14 grams / 32.0 g/mol

Moles oxygen = 0.2231 moles

Step 4: Calculate the limiting reactant

For 2 moles hexane we need 19 moles O2 to produce 12 moles CO2 and 14 moles H2O

Oxygen is the limiting reactant. It will completely be consumed ( 0.2231 moles). Hexane is in excess. There will react 2/19 * 0.2231 = 0.02348 moles

There will be porduced 12/19 * 0.2231 = 0.1409 moles CO2

Step 5: Calculate mass CO2

Mass CO2 = moles CO2 * molar mass CO2

Mass CO2 = 0.1409 moles * 44.01 g/mol

Mass CO2 = 6.20 grams

We can produce 6.20 grams of CO2