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1.0Moles of AL and 1.5 Mol of oxygen what is the empirical formula?
Wiki User
∙ 13y ago
Al2O3.
Wiki User
∙ 13y ago
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Determine the empirical formula what compound if a sample contains 0.104 mol K 0.052 mol C and 0.156 mol O?
Kc2o4
Is c2h4o2 a empirical formula?
Yes, it LOOKS like an empirical formula BUT it is NOT a correct one:Either C9H20 or C8H18 are correct (both are saturated alkanes) but not C8H20
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 formula mass of barium flouride?
Barium fluoride is BaF2. Its empirical formula is BaF2 as well. Hence, its formula mass is same as its molecular mass i.e.175.34g/mol
A compound formed of 0.059 mol hydrogen and 0.94 mol oxygen has a molecular mass of 34.0 gmole What is the molecular formula of this compound?
h2o2
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 molecular formula of a compound with the empirical formula NH2Cl and molar mass of 51.5g mol?
Nh2cl
Determine the empirical formula what compound if a sample contains 0.104 mol K 0.052 mol C and 0.156 mol O?
Kc2o4
What is the formula mass for tin sulfate?
Tin sulfate is made out of the elements tin, sulfur and oxygen. The mass numbers of tin, oxygen and sulfur are 117, 16 and 32 respectively. Therefore the molecular weight of the empirical formula is 215 g/mol.
Is c2h4o2 a empirical formula?
Yes, it LOOKS like an empirical formula BUT it is NOT a correct one:Either C9H20 or C8H18 are correct (both are saturated alkanes) but not C8H20
Empirical formula of a compound that contains 85.6 percent carbon and 14.4 percent?
Hypothetically, 100g of this substance will contain 52.1 g carbon, 13.2 g hydrogen and 34.7 g oxygen. Dividing these by their respective molar masses gives the amount in moles of each element. These are 4.34 mol, 13.1 mol, and 2.17 mol respectively. Divide all amounts given by the smallest non-integer amount, then multiply by whole numbers until the simplest ratio is found. These are 2 mol, 6 mol, and 1 mol respectively. The empirical formula of ethanol is C2H6O.
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.
If 1.164g of iron fillings reacts with chlorine gas to give 3.384 g of iron chloride what is the empirical formula of the compound Use the mole ratio method.?
1.164 g Fe / 55.85 g/mol = 0.02084 mol Fe (3.384 g - 1.164 g) Cl / 35.45 g/mol = 0.06262 mol Cl ratio of Fe : Cl = 1 : 3 empirical formula = FeCl3
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 is the formula of a molecule of oxygen?
The formula of an oxygen molecule is O2 (2 is a subscript but now WA doesn't permit to write a subscript).15.9994 g/mol is the molecular mass of oxygen. Formula mass is a sum of atomic mass of atoms in the molecule. In O2 there are two oxygen so it will be about 32g/mol
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 formula mass of barium flouride?
Barium fluoride is BaF2. Its empirical formula is BaF2 as well. Hence, its formula mass is same as its molecular mass i.e.175.34g/mol
