Final answer:
To calculate the mass of propane required to produce 50g of water through combustion, you must use the balanced chemical equation for propane's combustion, determine the number of moles of water produced, and then use stoichiometric ratios to find the corresponding mass of propane.
Step-by-step explanation:
The question you are asking pertains to the stoichiometry of a chemical reaction, specifically, the combustion of propane to produce water. To solve this problem, you would need to write and balance the chemical equation for the combustion of propane, C3H8, and use stoichiometric ratios from the balanced equation to determine the mass of propane that would react with oxygen to produce 50g of water. However, there is a typo in the formula you've provided; it should be C3H8, not C2H. Assuming you are seeking to find the mass of propane required to produce 50g of water, the balanced equation would be:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l)
Using the molar mass of water (18.02 g/mol), you can calculate the number of moles of water produced from 50g and then use the stoichiometric ratio to find the corresponding moles of propane required. Afterwards, convert the moles of propane to mass by using the molar mass of propane (44.10 g/mol).