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Relative molecular mass is obtained by summing up the atomic masses of atoms in the formula. The gram molecular mass denotes the mass of a mole of the substance in grams. Both of them are same in number.
As they are isobars, they have the same relative molecular mass.
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.
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
the formula is no. moles is mass / molecular mass. As the number of moles is 1, the mass required will be exactly the same as the molecular mass, which is 58.32g
They have the same relative molecular mass
Technically... not really. It would perhaps be more accurate to use the terms formula mass and molecular mass rather than formula weight and molecular weight. This because in physical terms, weight is a force while mass is a measure of the amount of substance in something.
The same as the molecular weight of the compound.
Proteins can have the same number of amino acids (and therefore same mass) yet be different proteins due to the different order of amino acids.
Since potassium chloride has the formula KCl and the mass of the lost electron from neutral potassium is negligible compared with the mass of the protons and neutrons in the potassium atom nucleus, the molecular mass of potassium in this compound is the same as the atomic mass of potassium, 39.098.
no, but sometimes they are equal.Added:Molecular mass differs from more common measurements of the mass of chemicals, such as molar mass, by taking into account the isotopic composition of a molecule rather than the average isotopic distribution of many molecules.As a result, molecular mass is a more precise number than molar mass.However it is more accurate to use molar mass on bulk samples. This means that molar mass is appropriate most of the time except when dealing with single molecules.
Both formulas are possible molecular formulas for the same empirical formula, CH2.