how many grams of H2O will be produced if 65.8 grams of CH3OH completely reacts?
To determine the amount of H2O produced from the reaction of CH3OH (methanol), we need to first understand the balanced chemical equation for the reaction. The balanced equation for the combustion of methanol is:
2CH3OH + 3O2 → 2CO2 + 4H2O
From the balanced equation, we can see that for every 2 moles of CH3OH that react, 4 moles of H2O are produced. Therefore, we need to convert the given mass of CH3OH (65.8 grams) to moles and then use the mole ratio to calculate the number of moles of H2O produced. Finally, we can convert the moles of H2O to grams.
1. Calculate the number of moles of CH3OH:
Number of moles of CH3OH = given mass / molar mass
The molar mass of CH3OH = (12.01 g/mol × 1) + (1.01 g/mol × 4) + (16.00 g/mol + 1) = 32.04 g/mol
Number of moles of CH3OH = 65.8 g / 32.04 g/mol
2. Determine the number of moles of H2O produced using the mole ratio from the balanced equation:
Number of moles of H2O = Number of moles of CH3OH × (4 moles H2O / 2 moles CH3OH)
3. Convert the number of moles of H2O to grams using the molar mass of water (H2O):
Mass of H2O = Number of moles of H2O × molar mass of H2O
The molar mass of H2O = 2(1.01 g/mol) + 16.00 g/mol = 18.02 g/mol
Therefore,
Mass of H2O = Number of moles of H2O × 18.02 g/mol
By plugging in the calculated values from steps 2 and 3, you will get the answer to your question, which is the mass of H2O produced when 65.8 grams of CH3OH completely reacts.