Gram Formula Mass
Gram Formula Mass
The idea of a mole is crucial to understanding Stoichiometry. Any element’s atomic weight in grams is equivalent to one mole of that element. Gram Formula Mass also has a lot of real-world applications in Physics. The Extramarks website and mobile application both have information on the Gram Formula Mass for students to learn more.
Gram Formula Mass
The Gram Formula Mass is the weight of one mole of an element, an ionic compound, or a molecular molecule. One mole of a substance contains 6.023 x 1023 atoms or molecules, depending on the sort of compound it is, or the Avogadro number.
The Gram Formula Mass is the atomic mass of one mole of an element, molecular compound, or ionic compound (a.k.a. molar mass). Therefore, while performing chemical calculations, the mole is a key number. The fields of Organic, Inorganic, and Physical Chemistry all make substantial use of this idea.
Amedeo Lorenzo Romano Italian scientist Carlo Avogadro was well known. He is most known for putting forth Avogadro’s law. According to the law, molecules will be present in equal numbers in equal quantities of gases under equal pressure and temperature.
In his honour, the number “Avogadro” is named. The quantity is referred to as Avogadro’s constant and has the value of 6.022140761023. The abbreviation NA is used to identify this basic SI unit.
Formula:
The precise Gram Formula Mass for determining a substance’s Gram Molecular Mass is:
Gram Formula Mass = the product of the solute’s mass and its formula. It is consistently given in terms of grammes per mole (g/mol).
However, Gram Formula Mass appears to be difficult to use the aforementioned formula in practical calculations. For practical purposes, people use a greatly simplified formula that is based on the idea that one mole of a substance will weigh the same as its atomic weight.
Therefore, each molecule can calculate its Gram Formula Mass using the aforementioned procedure. In order to solve such issues, it will be helpful to understand the atomic weights of the various elements.
The calculations linked to the Gram Formula Mass are a small portion of considerably larger calculations in competitive tests. Therefore, it is helpful to have in mind the Gram Formula Mass of several common chemicals, such as Carbon Dioxide, Carbon Monoxide, Methane, etc., to save time. Students must practice making quick conversions from moles to mass and vice versa so that they are adept at calculating the quantities during the actual exam. The Gram Formula Mass concept can be attained with continued practice.
Solved Examples for Gram Formula Mass
Q1: As an example, consider the compound ammonium phosphate, with the formula (NH4)3PO4.
Solution: To start, count how many atoms of each element are in the compound:
N: three atoms of nitrogen
Water (H): 12 Atoms
An atom of Phosphorus (P)
Oxygen(O) has four atoms.
Next, multiply the atomic weight of each element by the number of its corresponding atoms for each element:
3 * 14 = 42 for nitrogen
Water: 12 * 1 = 12
Phosphorous: 1 x 31 equals 31
Oxygen: 4 times 16 is 64.
Thus, 42 + 12 + 31 + 64 = 149 g/mol will be the total Gram Formula Mass.
Q2: What is the mass in grams of 1 mole of KAl(SO4)2.12H2O?
Solution:
1 K = 39 1 Al = 27\s2(SO4) = 192 = 2(32 + 16 × 4)
12 H2O = 216 = 12(2 + 16)
Therefore, 1 mole equals 474 grams in the gramme formula.
Q3: Calculate the mass of the compound H2SO4 using the gramme formula.
Solution:
H2SO4 is a chemical that students have.
Calculate the atomic weight of each element and multiply it by the number of atoms of each element that are present in the compound.
2 hydrogen atoms equal 2 1 = 2g.
Sulfur has the formula 1 32 = 32 grammes.
4 oxygen atoms = 4 x 16 = 64g
The total molecular mass of the molecule in grammes = Gram Formula mass
= 2 + 32 + 64
= 98 g
