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2:21 B 81% Analysis by mass of a compound containing carbon, hydrogen, oxygen and nitrogen only...
A compound of molar mass 166 contains only carbon, hydrogen, oxygen, and bromine. Analysis shows that a sample of the compound contains six times as much carbon as hydrogen, by mass. Part A Calculate the molecular formula of the compound. Express your answer as a chemical formula. Enter the elements in the order: C, H, O, Br. C6H7O2Br5
A compound containing carbon, hydrogen and oxygen has been analyzed. It contains 69.72% of carbon and 18.58% of oxygen. If the molecular weight of the compound is 86.13, what is its molecular formula? NOTE: Write the compound in the form (CXHYOZ), where X, Y and Z are whole numbers.
5. 74.1% carbon, 8.6% hydrogen, & 17.3% nitrogen by mass. Its molar mass = 160 g/mol. 6. 59.0% carbon, 7.1% hydrogen, 26.2%oxygen, & 7.7% nitrogen by mass. Its molar mass = 180 g/mol. Find the molecular formula of a compound given: 7. 212.1 g sample with 42.4 g hydrogen and 169.7 g carbon. Molar mass = 30.0 g/mol 8. Carbon & Hydrogen containing compound sample with molar mass = 114.26 g/mol. 1 mole of the sample contains 18.17 g hydrogen....
Combustion of a 1.025 g sample of a compound containing only carbon, hydrogen and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical and molecular formulas of the sample compound, if its molecular weight has been roughly determined to be 363 g/mol by mass spectrometer?
A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 15.48 mg CO2 and 7.39 mg H20. The molar mass of the compound is 182.2 g/mol What are the empirical and molecular formulas of the compound? (Enter the elements in the order: C, H, O) The empirical formula: The molecular formula
A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 15.48 mg CO2 and 7.39 mg H2O. The molar mass of the compound is 182.2 g/mol. What are the empirical and molecular formulas of the compound? (Enter the elements in the order: C, H, O.) The empirical formula:? The molecular formula:?
Combustion analysis of 0.6943 g of an unknown compound containing carbon, hydrogen, and oxygen, produced 1.471 g CO2 and 0.226 g H2O. Determine the molecular formula, given the molar mass is 166 g/ mol.
1. Dioxybenzanone is a compound found in sunscreen, and only contains carbon, oxygen, and hydrogen. Analysis of the compound found that it contains 4.92% hydrogen, 26.18% oxygen. What is the empirical formula of the compound? (4 pts) 2. The ionization energy of oxygen is found to be less than that of nitrogen. Is this to be expected? Explain why or why not. (4 pts)
A compound containing carbon, hydrogen, and perhaps other elements shows a mass spectrum with a molecular ion at 115. Suggest at least 2 possible structures for the compound. In the molecular ion region of the mass spectrum, a compound containing carbon, hydrogen, and perhaps other elements gives peaks at 90 and 92. The 92 peak is about 1/3 the height of the 90 peak. Give at least 2 possible structures for the compound.
2.516 g of a compound containing carbon, hydrogen and oxygen (CXHYOZ) is subjected to combustion analysis. The results show that 3.082 g of CO2 and 2.705 g of H2O were produced. (i). What is the empirical formula for the compound? (ii). If the molecular weight of the compound is 160.2 g/mol, what is the molecular formula of the compound?