A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume you have a 100.-g sample...
A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume you have a 100.-g sample of this compound. The molar mass of the compound was found to be 30.069 g/mol. What is the molecular formula?
Express your answer as a chemical formula.
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A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume
you have a 100.-g sample...
A compound of molar mass 166 contains only carbon, hydrogen, oxygen, and bromine. Analysis shows that...
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
5. 74.1% carbon, 8.6% hydrogen, & 17.3% nitrogen by mass. Its molar mass = 160 g/mol....
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....
I have an unknown organic compound containing carbon, hydrogen and oxygen. Combustion analysis of 4.05 g...
I have an unknown organic compound containing carbon, hydrogen and oxygen. Combustion analysis of 4.05 g sample of the unknown produced 8.07 g CO2 and 3.76 g H2O. The molar mass of the unknown was determined to be 180 +/- 4 g/mol. What is the molecular formula of the unknown?
A 0.5998 sample of a new compound with a molar mass of 93.12 g/mol was analyzed...
A 0.5998 sample of a new compound with a molar mass of 93.12 g/mol was analyzed and found to have 0.2322g of carbon,some hydrogen,and 0.3091g of oxygen. What is the formula for the compund?
1.)) An unknown compound containing carbon, hydrogen and oxygen is combusted. If 25.000 g of the...
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 1.802 gram sample of unknown compound contains 0.721 grams of carbon, 0.121 grams of hydrogen...
A 1.802 gram sample of unknown compound contains 0.721 grams of carbon, 0.121 grams of hydrogen and 0.960 grams of oxygen. The compound has a molar mass of 180.2 g/mol. Determine the empirical formula of the compound and the molecular formula. Show all work.
3.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps...
3.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 160. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass 5.78 g carbon dioxide 1.58 g water Use this information to find the molecular formula of X.
6.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar...
6.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 78. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product carbon dioxide mass 22.01 g water 4.50 g Use this information to find the molecular formula of X, x 6 ?
7.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar...
7.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 26. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: mass product carbon dioxide water 23.70 g 4.85 g Use this information to find the molecular formula of X. x 6 ?
6.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps...
6.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 26. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 20.31 g water 4.16 8 Use this information to find the molecular formula of X.
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....
3.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 160. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass 5.78 g carbon dioxide 1.58 g water Use this information to find the molecular formula of X.
6.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 78. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product carbon dioxide mass 22.01 g water 4.50 g Use this information to find the molecular formula of X, x 6 ?
7.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 26. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: mass product carbon dioxide water 23.70 g 4.85 g Use this information to find the molecular formula of X. x 6 ?
6.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 26. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 20.31 g water 4.16 8 Use this information to find the molecular formula of X.
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