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A gaseous binary compound has a vapor density that is 1.94 times that of oxygen at the same temperature and pressure. When 1.39 g 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
(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?
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Chapter 2 Solutions
Bundle: Principles of Modern Chemistry, 8th + OWLv2, 1 term (6 months) Printed Access Card
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- Use the References to access important values if needed for this question. A binary compound of oxygen and an unknown element, X, has the formula X,0 and is 53.55 mass % oxygen. (a) What is the atomic weight of element X? u (b) What is the symbol for the element on the periodic table? X = (c) Is the element X a metal or not? (d) Is the compound X20 likely to be ionic or covalent? (e) What is the name of the compound? Submit Answer 5 question attempts remainingarrow_forward2.90 grams of phosphorus is burned in the presence of oxygen and forms 5.14 grams of a phosphorus oxide. What is the emperical formula of the phosphorus oxide formed? Then write a balanced equation for the formation of the phosphorus oxide.arrow_forwardA binary compound of oxygen and an unknown element, x, has the formula XO and is 39.70 mass % oxygen. (a) What is the atomic weight of element x ? u (b) What is the symbol for the element on the periodic table? x = (c) Is the element x a metal or not? (d) Is the compound xO likely to be ionic or covalent? (e) What is the name of the compounc 4 question attemptsarrow_forward
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