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.
100gm of compound contains
C = 69.72gm*1/12.01*mol/gm= 5.8
O = 18.58gm*1/16mol/gm = 1.16
H = 100-(69.72+18.58) = 11.7gm*1/1.01 mol/gm = 11.6
Mole ratio:
Dividing by smallest mol 1.16
C =5.8/1.16=5
O=1.16/1.16=1
H=11.6/1.16=10
So mol ratios give empirical formula C5OH10
Empirical formula weight = 5*12.01+1*16+10*1.01= 86.16 which is nearly equal to the molecular weight 86.13
So molecular formu
la is C5OH10
A compound containing carbon, hydrogen and oxygen has been analyzed. It contains 69.72% of carbon and...
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?
20) A compound was analyzed and found to be 47% Carbon, 11% Hydrogen and 42% Oxygen, What is its Empirical Formula? What is its molecular formula if its molecular weight is 304 g/mole?
20) A compound was analyzed and found to be 47% Carbon, 11% Hydrogen and 42% Oxygen, What is its Empirical Formula? What is its molecular formula if its molecular weight is 304 g/mole?
A compound is analyzed and found to contain 68.54% carbon, 8.63% hydrogen, and 22.83% oxygen. The molecular weight of this compound is known to be approximately 140 g/mol. What is the empirical formula? What is the molecular formula?
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?
1.)) An unknown compound containing carbon, hydrogen and oxygen is combusted. If 25.000 g of the compound produced 61.024 g of CO2 and 24.981 g of H2O, what is the empirical formula of the compound? 2.)) If the molar mass of this compound is 72.1 g/mol, what is 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 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:?
A compound that contains only carbon, hydrogen, and oxygen is 45.3 % C and 9.43 % H by mass. What is the empirical formula of the substance? Enter the correct subscript for each atom using the smallest whole number. Its not C1H3O1
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