Final answer:
To find the amount of water produced from 50g of methanol, calculate the moles of methanol, determine the stoichiometric relation with water in the reaction, and convert the resulting moles of water to grams. This results in 14.0625 grams of water produced.
Step-by-step explanation:
The student is tasked with determining the amount of water produced when 50 grams of methanol (CH₃OH) reacts according to the given chemical equation. First, we need to find the number of moles of CH₃OH that 50 grams corresponds to by using its molar mass, which is 32 g/mol.
Step 1: Calculate the moles of CH₃OH.
Number of moles = mass (g) / molar mass (g/mol) = 50 g / 32 g/mol = 1.5625 mol
According to the chemical equation, 2 moles of CH₃OH yield 1 mole of H₂O. Thus, the number of moles of water produced will be half the number of moles of CH₃OH.
Step 2: Relate moles of CH₃OH to moles of H₂O.
Moles of H₂O = 1.5625 mol CH₃OH × (1 mol H₂O / 2 mol CH₃OH) = 0.78125 mol H₂O
Now, we can convert the moles of water to grams using its molar mass of 18 g/mol.
Step 3: Convert moles of H₂O to grams.
Mass of H₂O = 0.78125 mol × 18 g/mol = 14.0625 g
Therefore, 50 grams of CH₃OH can produce 14.0625 grams of water.