Final answer:
Without a given chemical reaction that details the stoichiometry between CaCN2 and H2O, it is not possible to calculate the mass of H2O produced from 12.85g of CaCN2.
Step-by-step explanation:
To determine how many grams of H2O would be produced from 12.85g of CaCN2, we first need to know the balanced chemical reaction. However, since no reaction is provided in the question, let us consider a common reaction where calcium cyanamide (CaCN2) can be used to produce water:
CaCN2 + 3H2O → CaCO3 + 2NH3
From the equation, for every mole of CaCN2, 3 moles of H2O are required. But as we're interested in the production of water, the reaction is not helpful without the corresponding stoichiometry. Since we do not have this information, we would not be able to calculate the mass of water produced without the proper reaction context.
Normally, one would calculate the molar mass of CaCN2, use it to find the number of moles of CaCN2 in 12.85g, and then use stoichiometry to find the moles and subsequently grams of H2O produced. However, in absence of the correct chemical reaction details, this calculation cannot be completed.