Final answer:
The moles of CO2 produced from 130g of H2O formed, the mole ratio from a balanced chemical equation is needed. For a generic hydrocarbon combustion, 7.22 moles of H2O would yield 4.81 moles of CO2, given a 3:2 H2O to CO2 ratio. None of the provided options match this correct calculation.
Step-by-step explanation:
The question is related to stoichiometry, which is a branch of chemistry that involves calculating the amounts of reactants and products in a chemical reaction. To find the moles of CO2 produced when 130g of H2O are formed, one must first consider the stoichiometry of the chemical reaction in question. Assuming the reaction is the combustion of a hydrocarbon or similar reaction yielding CO2 and H2O, we'll find a balanced chemical equation to establish the mole ratio between H2O and CO2.
For illustrative purposes, we can consider the combustion of ethane (C2H6), which has the equation 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O. From this, the mole ratio of H2O to CO2 is 6:4 or 3:2. Now we divide the mass of H2O formed by its molar mass, 18.015 g/mol, to obtain moles of H2O: 130g / 18.015 g/mol = 7.22 moles of H2O. Since the mole ratio is 3:2, we multiply the moles of H2O by 2/3 to get the moles of CO2.
Calculations: 7.22 moles H2O (2/3) = 4.81 moles CO2
Thus, none of the provided options are correct. An accurate answer can be approximated or calculated using a balanced chemical equation relevant to the scenario given.