Question

Upon ignition, methanol (CHsOH) burns readily in air. How many total moles of products are formed if 60.0 mL of methanol (D 0.850 g/mL) react with 18.7 L of oxygen at 37°C and 1.72 atm?

Answer 1

To calculate the total moles of products from the combustion of methanol, we use density to find the mass of methanol, convert it to moles, apply the ideal gas law for oxygen, and use the stoichiometry of the balanced chemical equation to determine the moles of CO2 and H2O produced.

Step-by-step explanation:

The question involves stoichiometry and gas laws to determine the total moles of products formed from the combustion of methanol in oxygen. First, the volume of methanol is converted to mass using the given density, then to moles using the molar mass of methanol.

The Ideal Gas Law (PV = nRT) is then used to calculate the moles of oxygen available. The balanced chemical equation for the combustion of methanol is CH3OH(l) + 1.5O2(g) → CO2(g) + 2H2O(g). Using the limiting reactant, the total moles of products are calculated, summing the moles of carbon dioxide and water produced in the reaction.