Question

Consider the reaction between 50.0 mL of liquid methanol(CH3OH; density = 0.850 g/mL) and 22.8 L ofO2 at 27°C and a pressure of 2.02 atm. The products of the reaction areCO2(g) and H2O(g).Calculate the number of moles of H2O formed if thereaction goes to completion.

_________mol

Answer 1

The number of moles of H2O formed in the combustion of methanol with oxygen, given the provided reactant quantities and conditions, is 2.487 moles.

Step-by-step explanation:

To calculate the number of moles of H2O formed in the reaction of liquid methanol (CH3OH) and oxygen (O2), we need to know the balanced chemical equation. The reaction is:

2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g)

First, we calculate the moles of CH3OH using its volume and density:

Now, we calculate the moles of O2 using the ideal gas law (PV=nRT)

According to the stoichiometry of the balanced equation, 2 moles of CH3OH react with 3 moles of O2 to produce 4 moles of H2O. Therefore, the limiting reactant must be identified to find the number of moles of H2O produced.

Using the stoichiometric ratios:The number of moles of H2O formed is 2.487.