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When 0.424g of iron powder is burned in an oxygen atmosphere 0.606g of a reddish brown oxide is obtained. Determine the empirical formula of oxide.?
The increased weight of 0.606 - 0.424 = 0.182 (g) must be due to oxygen. Since Fe has atomic weight of 55.845, and Oxygen 16.00. Hence in 0.606g reddish brown oxide, 0.424g iron is 0.424/55.845 Mol = 0.00759 Mol, and 0.182g oxygen is 0.182/16.00 Mol = 0.01138 Mol. Since 0.01138/0.00759 = 1.4982 ≈ 1.5, the emperical must be Fe2O3.
What else can I help you with?
What is the empirical formula of C3H6O3?
The empirical formula of C3H6O3 is CH2O. This is obtained by dividing the subscripts in the molecular formula by the greatest common factor.
Empirical formula of C3H6?
C3H6 is an empirical formula for propene.
How To Determine The Empirical Formula From 46.25 grams Sample That Contains 14.77 grams Of K 9.06 Of O 22.42 grams Of tin.?
To determine the empirical formula, first calculate the moles of each element present by dividing the given masses by their respective molar masses. Then, divide each mole value by the smallest mole value obtained. Finally, round the resulting ratio to the nearest whole number to determine the subscripts required for the empirical formula. In this case, the empirical formula would be K2O2Sn.
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 the compound below C10H25O5?
C2H5O. Empirical formula is the simplest integer ratio of atoms.
What is the empirical formula of C3H6O3?
The empirical formula of C3H6O3 is CH2O. This is obtained by dividing the subscripts in the molecular formula by the greatest common factor.
Empirical formula of C3H6?
C3H6 is an empirical formula for propene.
How To Determine The Empirical Formula From 46.25 grams Sample That Contains 14.77 grams Of K 9.06 Of O 22.42 grams Of tin.?
To determine the empirical formula, first calculate the moles of each element present by dividing the given masses by their respective molar masses. Then, divide each mole value by the smallest mole value obtained. Finally, round the resulting ratio to the nearest whole number to determine the subscripts required for the empirical formula. In this case, the empirical formula would be K2O2Sn.
What is empirical formula of s2cl2?
The empirical formula of S2Cl2 is SCl. This is obtained by reducing the subscripts of each element in the compound to their simplest ratio.
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 the compound below C10H25O5?
C2H5O. Empirical formula is the simplest integer ratio of atoms.
What information is needed to determine molecular formula?
the empirical formula and the molar mass
What Process of using empirical formula and the value for experimental molar mass to determine the molecular formula?
The empirical formula is the formula in its most simplified terms. The molecular formula is how many moles there actually are (the empirical formulat multiplied by a factor).
How do you calculate Molecular formula from empirical formulaWhat could you do with that information to determine that the empirical and molecular formulas are related to one another by a factor of 6?
In order to find molecular formula from empirical formula, one needs to know the molar mass of the molecular formula. Then you simply divide the molar mass of the molecular formula by the molar mass of the empirical formula to find out how many empirical formulae are in the molecular formula. Then you multiply the subscripts in the empirical formula by that number.
How does one determine a molecular formula from the empirical form?
molar mass of unknown/molar mass of empirial = # of empirical units in the molecular formula. Example: empirical formula is CH2O with a molar mass of 30. If the molar mass of the unknown is 180, then 180/30 = 6 and molecular formula will be C6H12O6
Choose the empirical formula?
To determine the empirical formula of a compound, you need the molar masses of its elements and their ratio in the compound. Calculate the ratio of the elements in terms of whole numbers, which will give you the empirical formula.
To determine the subscript of an element in a molecular formula the empirical mass must be multiplied by the actual mass?
The actual mass must be divided by the empirical mass. This was derived from the following equation: (subscript)(empirical formula) = (molecular formula) subscript = (molecular formula)/(empirical formula)
