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If a compound has an empirical formula of CH and a mass of 26 grams what is the molecular formula?
Wiki User
∙ 15y ago
First, add together the atomic masses of the elements:
C- 12.0
H- 1.00
_______
13.0
Now put it into the following formula:
x(added Atomic Mass) = molecular weight
13.0x = 26.0
Then find x
x= 2
Take the x value and multiply it with the number of atoms in the empirical formula/
C1H1 * 2 = C2H2
The final answer is the actual molecular formula C2H2 or Acetylene
Wiki User
∙ 15y ago
Anonymous
Wiki User
∙ 15y agoFirst, find the atomic masses of the elements and add them together:
C - 12.0
H - 1.00
_____
13.0 g
Use this formula to find the actual molecular formula:
x(added atomic mass) = molar mass of compound
x(13.0) = 78.0 g
Divide the added atomic mass to get x = #:
x = 6
Take your x value and multiply the number of atoms in the empirical formula by it:
C1H1 * 6 = C6H6
The final result is the actual molecular formula.
Wiki User
∙ 11y agothe mass of 1.0 mole of the simplest ratio 'molecule' (CH) is (C) 12 + (H) 1 = 13 g for 1.0 mole (CH)
78 g = 1 mole (CxHx) , so x = 78 / 13 = 6 so the molecular formula is C6H6
Wiki User
∙ 12y agoI'm confused myself
maybe not sure but i think you would... iidk
Wiki User
∙ 13y agoCH = 13 so 78/13 = 6 The compound is C6H6 = benzene (most likely).
Wiki User
∙ 6y agoThe molar mass of hexane is 86,18 g.
Wiki User
∙ 11y agoC3h3
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What is the molecular formula of a compound with an empirical formula of C4H9 and a gram formula mass of 114 grams mole?
C8h18
What is the molecular formula of a compound given the molar mass of the compound is 162.27 grams and the empirical formula is C2H3?
The empirical mass is C2H3 2 x 12 = 24 3 x 1 = 3 24 + 3 = 27 So divide 27 into 166.01 Hence 162.27 / 27 = 6.01 ~ 6 So multiply each atom in the empirical formula by '6' Hence Empirical C2H3 Molecular C12H18
How does one determine a molecular formula from empirical formula?
molar mass over grams of elementThe above answer is somewhat correct. In order to find the molecular formula when given the empirical formula, you must first find the molar mass of the empirical formula.MOLAR MASS# atoms element A x Atomic Mass element A (Periodic Table) = mass A# atoms element B x atomic mass element B (periodic table) = mass B... etc.Add up all of the mass values found above and you have the molar mass.Then, after you have found the empirical formula's molar mass, you divide the molar mass of the molecular formula by the empirical formula's molar mass (solving for n).MOLECULAR FORMULA EQUATION: N (Empirical formula) (read as N times empirical formula) where:N = Molar mass substance---- Molar Mass emp. form.
Would you expect an empirical formula to be the same even though different masses used?
This question refers to masses of elements as opposed to their molecular formulas. In the example of MgCl2 there will always be Mg in a 1:2 molar ratio with chlorine. Molar mass gives the relationship.
What is the chemical formula for trisulfur phosphide?
Diphosphorus trisulfide is comprised of 2 phosphorus (P) and 3 sulfur atoms. its molecular formula is this P2S3 and it has a molecular mass of 148-grams per mole.
What is the molecular formula of a compound with an empirical formula of C4H9 and a gram formula mass of 114 grams mole?
C8h18
What is the molecular formula of a compound that has an empirical formula of c2oh4 and a molar mass of 88 grams per mole?
C4O2H8
What is its molecular formula if the molar mass of the compound is 199.55 grams per mole?
Cannot answer this question without knowing the EMPIRICAL formula.
What steps are used to convert an empirical formula into a molecular formula?
By determining the molecular mass, then dividing the molecular mass by the formula mass of the empirical formula to determine by what integer the subscripts in the empirical formula must be multiplied to produce the molecular formula with the experimentally determined molecular mass.
How do you calculate the molecular formula of a substance which contain 80 percent C and 20 percent H?
You can only calculate the empirical formula because you do not have a mass of this compound given. To do the empirical formula assume 100 grams and change percent to grams. Get moles. 80 grams Carbon (1 mole C/12.01 grams) = 6.66 moles C 20 grams hydrogen (1 mole H/1.008 grams) = 19.84 moles H the smallest becomes 1 in the empirical formula and the other number is divided by it, Thus; H/C 19.84 moles H/6.66 moles C = 2.9, which we call 3 so, CH3 --------------- is the empirical formula To get the molecular formula tour question needed to read; How to calculate molecular formula from such ans such mass of compound with these percentages of elements, Which, of course, your question did not provide. Then you would have divided that given mass by the mass total of the elements of the empirical formula, got a whole number by which you would have multiplied the numbers of your empirical formula to get molecular formula.
What is the molecular formula of fructose with C 40 percent H 6.72 percent O 53.28 percent?
We assume 100 grams and turn those percentages into grams and find moles of species. 40 grams carbon (1 mole C/12.01 grams) = 3.33 moles C 6.72 grams hydrogen (1 mole H/1.008 grams) = 6.67 moles H 53.28 grams oxygen (1 mole O/16 grams) = 3.33 The smallest mole number is 1, so we have two small numbers. Divide the large number by the small. 6.67/3/33 = 2 so.............. CH2O is the empirical formula. You did not state that you had a quantity of this compound ( such as 60 grams, or whatever ), so the molecular formula can not be found from this info. C6H12O6 is of course the molecular formula. To find the molecular formula you need a mass of the compound aside from the simple percentages. Then you find, as we have done, the empirical formula. you divide the mass given by the mass of the empirical formula and then take that quotient and multiply it times the empirical formula. In this case (CH2O) * 6 = C6H12O6, the molecular formula
What is the molecular formula of a compound given the molar mass of the compound is 162.27 grams and the empirical formula is C2H3?
The empirical mass is C2H3 2 x 12 = 24 3 x 1 = 3 24 + 3 = 27 So divide 27 into 166.01 Hence 162.27 / 27 = 6.01 ~ 6 So multiply each atom in the empirical formula by '6' Hence Empirical C2H3 Molecular C12H18
What is the molecular formula of a substance that has an empirical formula of C2H5 and a molecular mass of 58 grams per mole?
If C2H5 was the molecular formula its molecular mass would be 29 ( 12 x 2 + 5 x 1) However, 29 x 2 = 58 the actual molecular mass. So we double up the atoms in C2H5 to C4H10 . C4H10 is the molecular formula.
An iron chloride compound contains 55.85 grams of iron and 106.5 grams of chlorine What is the most likely empirical formula for this compound?
Fe3Cl
What is the most likely empirical formula for a compound that contains 55.85 grams of iron and 106.5 grams of chlorine?
FeCl3
Ibuprofen a common pain remedy has an empirical formula of C7H9O and a molar mass of approximately 218.078 grams per mole. What is the molecular formula of ibuprofen?
molar mass of empirical = 7x12 + 9x1 + 16 = 109 g/mole218.078/109 = 2 so there are 2 empirical formulae in 1 molecular formulaThe molecular formula is therefore C14H18O2
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)
