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What is the empirical formula of ascorbic acid given that the pseudoformula is C 3.407 H 4.53 O 3.406?
Wiki User
∙ 10y ago
The nearest, almost round figures are found when you double the pseudo- (experimentally found ratio-) numbers:
- C 3.407*2=6.814, best rounded: 7
- H 4.53*2=9.106, best rounded: 9
- O 3.406*2=6.812, best rounded: 7
However this is not according to ascorbic acid's ratio 3:4:3 (C6H8O6) and even further away from the dehydro-ascorbic acid ratio 1:1:1: (C6H6O6)
Wiki User
∙ 10y ago
Wiki User
∙ 13y agoC3h4o3
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How does one determine a molecule formula from the empirical formula?
The density or some other information must be given that allow you to find the molar mass. Calculate the empirical formula mass. Divide molar mass by empirical formula mass. This answer is multiplied by all subscripts of the empirical formula to get the molecular formula.
What is the empirical formula for butane?
Well you know that Butanoic Acid's Molecular formula is C3H7COOH, and Empirical formula is a compound showig the simplest ratio of numbers of atoms of each element in the compound. Now the question is, can you simply C3H7COOH ? Nope! Then the Empirical formula is also C3H7COOH
What is the molecular formula of a compound given that molar mass of the compound is 30.04 gram and the empirical formula is NH?
The molecular formula of this compound is N2H2. This is obvious because the empirical formula of a compound is the lowest positive integer ratio of atoms present.
What is this empirical formula - C5H8NO4?
C4h5n2o
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.
How do you know when to solve for a empirical formula?
If it tells you to find the empirical formula when percent composition is given or if the mass of each element is given in a specific compound.
What is the empirical formula for C3H5?
The empirical formula is C3H5. The answer does not change from the given form because there is no common denominator to divide by.
How does one determine a molecule formula from the empirical formula?
The density or some other information must be given that allow you to find the molar mass. Calculate the empirical formula mass. Divide molar mass by empirical formula mass. This answer is multiplied by all subscripts of the empirical formula to get the molecular formula.
Which could represent the empirical and the formula of a given compound?
The empirical formula is representative for the chemical composition of a compound; the structural formula is representative for the spatial structure of the compound.
Explain why the percent composition of certain compounds are not sufficient to determine the compounds molecular formulas?
Because unlike the empirical formula, the molecular formula does not have to be the simplest ratio.If by chance you are given the percent composition of the elements in a substance, you could calculate the empirical formula and then the empirical formula's mass. However, the molecular formula equation is molecular formula= (empirical formula)n, where n is the mass of the molecular formula divided by the mass of the empirical formula. You would, therefore, need to know the mass belonging to the molecular formula, which you are not given.
What is the chemical formula for silcon chloride?
It creates a covalent lattice and the empirical formula can be given as SiCl4.
What is the empirical formula for butane?
Well you know that Butanoic Acid's Molecular formula is C3H7COOH, and Empirical formula is a compound showig the simplest ratio of numbers of atoms of each element in the compound. Now the question is, can you simply C3H7COOH ? Nope! Then the Empirical formula is also C3H7COOH
What is the properly written empirical formula of a compound of molecular formula C6H12 with a molar mass equal to 84.16 gram per mol?
The information about the actual molar mass is superfluous. Given any molecular formula, the corresponding empirical may be obtained by dividing all the subscripts in the molecular by the largest integer that yield an integer quotient for each subscript. In the given formula, the empirical formula is CH2.
What is the molecular formula of a compound given that molar mass of the compound is 30.04 gram and the empirical formula is NH?
The molecular formula of this compound is N2H2. This is obvious because the empirical formula of a compound is the lowest positive integer ratio of atoms present.
How is a molecular formula determined?
There are 4 step to determine molecular formula, which are given bellow Step:1:- Find empirical formula Step:2:- Find empirical formula mass Step:3:- Find n n=molecular mass/empirical formula mass Step:4:- now find molecular formula to find molecular formula molecular formula(empirical formula)n
What is this empirical formula - C5H8NO4?
C4h5n2o
What is the empirical formula for a Compound with the molecular formula C16H12CI2O2?
The formula as written, including a capital "I", is already an empirical formula, since it shows a total of 7 carbon atoms and none of the other subscripts is integrally divisible by 7. However, the formula may have been intended to be written C16H12Cl2O2. In that instance, all the subscripts can be integrally divided by 2 to given an empirical formula of C8H6ClO.
