1. The problem statement, all variables and given/known data "A gaseous binary compound has a vapor density that is 1.94 times that of oxygen at the same temperature and pressure. When 1.39g of the gas is burned in an excess of oxygen, 1.21 g water is formed, removing all the hydrogen originally present. (a) Estimate the molecular mass of the gaseous compound. (b)How many hydrogen atoms are there in a molecule of the compound? (c) What is the maximum possible value of the atomic mass of the second element in the compound? (d) Are other values possible for the atomic mass of the second element? Use a table of atomic masses to identify the element that best fits the data. (e) What is the molecular formula of the compound? " p.47 question 29 out of "Principles of Modern Chemistry" (Authored by: Oxtoby Gillis Campion). 3. The attempt at a solution My attempt at this solution I do not believe is worth writing. This is not work assigned from a college course, I am simply trying to study chemistry independently. With this question, I have not been able to find an effective approach to yield a correct solution. Help provided will be greatly appreciated.