Al2O3.
Kc2o4
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
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.
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
h2o2
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.
Nh2cl
Kc2o4
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.
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
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.
The formula of NO2 has a molecular weight of 46 g/mol. Your compound has a molecular weight of 92 g/mol. As you can see the molecular weight of the compound is twice that of the empirical formula. Therefore the molecular formula of your compound is:2 *(NO2) ---> N2O4
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
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.
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
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.
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