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What is the empirical formula of a substance that is 53.3 percent c 15.5 percent h and 31.1 percent n by weight?
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∙ 13y ago
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∙ 13y ago
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Empirical and molecular formulas?
The Empirical formula of Al2Br6 is AlBr3.
What is the empirical formula of a compound that contains 59.9 percent titanium and 40.1 percent oxygen?
Ti - atomic weight = 47.867 O - atomic weight = 16.0 59.9/47.867 = 1.25 40.1/16 = 2.50 2.50/1.25 = 2 therefore 1 Ti atom and 2 O atoms so TiO2
What is the empirical formula of a compound that is 50.7 percent antimony and 49.3 percent selenium by weight?
We assume 100 grams of the compound and turn those percentages into grams and get the moles. 50.7 grams antimony (1 mole Sb/121.8 gram) = 0.41626 moles antimony ================================ Now, the smallest mole number (antimony) becomes 1 and the other number is divided by it(antimony) to get the empirical numbers. 0.62467 moles Se/0.41626 moles Sb = 1.5 ----------------so, this happens sometimes and this is what we do (SbSe1.5)*2 = Sb2Se3 -----------------The empirical formula Antimony selenide
An unknown pesticide is made up of 18.28 percent carbon 0.77 percent hydrogen and 80.95 percent chlorine What is the empirical formula of the pesticide?
I assume that these are weight percents. If so, assume you have 100 g of the substance. Then divide each by the molecular weight to find the number of moles of C, H, & Cl.C: 18.28 g * (1 mole C/12.011 g C) = 1.522 moles CH: 0.77 g * (1 mole H/1.008 g H) = 0.764 moles HCl: 80.95 g * (1 mole Cl/35.453 g Cl) = 2.283 moles ClNext find the ratio of moles of C to H to Cl. To do this divide each by the smallest number of moles from the list, in this case it will be hydrogen.C: 1.522/0.764 = 1.99 (round it to 2)H: 0.764/0.764 = 1.00Cl: 2.283/0.764 = 2.99 (round it to 3)So your empirical formula of the pesticide should be C2HCl3
What is the formula of equivalent weight?
Equivalent weight = Molar mass of a substance/electrical charge of the ions (positive or negative) formed in solution Also the equivalent weight of a substance react with 1 mole of hydrogen. Today this expression is rarely used.
Can you determine the molecular formula of a substance from its percent composition?
Not completely. The empirical formula of a substance can be determined from its percent composition, but a determination of molecular weight is needed to decide which multiple of the empirical formula represents the molecular formula.
How to calculate empirial formula from molecular formula?
Calculate the empirical formula weight. Find the ratio of the molecular weight to the empirical formula weight. (n= molecular weight/ empirical formular weight). Multiply each subscript of the empirical formula by n.
What is the importance of percentage composition?
Percent composition can be used to calculate the percentage of an element/compound in a mixture. From the percent composition, you can also find the empirical formula. And from the empirical formula you can find the actual molecular weight.
What is the empirical formula of a hydrocarbon containing 85.7 percent carbon and 14.3 percent hydrogen?
The molecular formula is C3H6 and the empirical formula is CH2. This compound is called propene or propylene, and it is a colorless gas.
How can you find the molecular formula of a compound when its percentage composition is given?
Yes, if you have some additional information, such as the molecular weight. For instance, the molecules C2H4 and C4H8 have exactly the same percent composition, but they are very different molecules. So you need some other information to tell them apart than the percent composition.Answer ExpandedThis is kind of a trick question. By knowing the percent composition, you would easily be able to determine its empirical formula, but molecular formula is a bit different. The molecular formula is the actual number of atoms in a molecule, so in order to find the specific molecular formula of a substance, you would also need to know how many grams there is of that substance.(This explains the difference between C2H4 and C4H8)
What is the empirical formula of a compound that is 4 percent sulfur and 6 percent oxygen by weight?
We can't tell. What's the other 90 percent? If you meant 40/60 instead... the mass of sulfur is twice that of oxygen, so a mass ratio of 40:60 is equivalent to an atom ratio of 1:3. The empirical formula would be SO3.
What is the molecular formula of a compound if the weight is of a unit of the compound is 120 and the empirical formula is C3H4?
C9h12
How do you find the empirical formula of a compound of uranium and fluorine that is composed of 67.6 percent uranium and 32.4 percent fluorine?
This compound is UF6. Atomic weight of uranium: 238,02891 Atomic weight of fluorine: 18,9984032 Molecular mass of UF6: ca. 352,04121
What is the empirical formula of a compound that is 40percent sulfur and 60percent oxygen by weight?
SO3
What is the Molar mass of empirical formula NO2?
The empirical mass of NO is 14 + 16 = 30 Divide 138 / 30 ~ = 4.5. The fact that the numbers are not whole number would suggest that the empirical formula is incorrect. However, if we use say NO2 as the empirical formula , then the empirical mass is 14 + 16 + 16 = 46 divide 138 /46 = 3 So NO2 has a formula of N3O6 . This substance does not exist, So it would suggest that the formula is 3NO2 (3/2)N2O4 . I would suggest that the original empirical formula is incorrect. and that the substance is either nitrogen dioxide (NO2) or dinitrogen tetroxide N2O4.
Empirical and molecular formulas?
The Empirical formula of Al2Br6 is AlBr3.
What is Formula of urea?
The Chemical formula of Urea is CO(NH2)2 its empirical formula is just the same as its chemical formula. Urea has a molecular weight of 60.06gm.
