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The average Atomic Mass of an element is the weighted average mass of an atom (including all its isotopes).
This is related to the molar mass, because molar mass is the weight of 1 mole of something (atoms, molecules, etc...).
1 mole = 6.022 x10^23 = avogardro's constant.
What else can I help you with?
Is the number of atoms in a sample directly related to the mass of that sample?
If the chemical composition of the sample is known, then the answer is yes. However, equal masses of platinum and magnesium, for example, contain quite different numbers of atoms, because the atomic mass of platinum is much higher than that of magnesium.
How is a mole related to the atomic mass?
The atomic mass, in grams, is the mass of one mole of atoms.
In addition to the atomic number what other numerical value appears in the square for each element in a periodic table?
Atomic Mass
Why is atomic mass not a constant number?
The atomic mass is the average of all of the different isotopes of the element present in the sample. Samles taken from aound the worlld for some elements have slightly different isotope ratios and therefore have different atomic masses.
Each element has its own characteristic atom in which a. the atomic weight is constant b. the atomic number is constant c. the mass number is constant?
b. the atomic number is constant. The mass number is not constant because there are isotopes of an element that have the same number of protons but different number of neutrons. Likewise, there are isotopes of the same element with different atomic weights.
Is it a lucky accident that avogadro's number of helium atoms weight exactly four grams?
No, it is not a lucky accident. An Avogadro's number of helium atoms do not weigh 4 grams: their mass is four grams and that is NOT the same thing. The mass is related to the atomic mass unit which is, essentially the number of protons and neutrons in an atom. More accurately, it is the weighted average for the atomic mass across the isotopes of the element - weighted according their abundance.
Is the number of atoms in a sample directly related to the mass of that sample?
If the chemical composition of the sample is known, then the answer is yes. However, equal masses of platinum and magnesium, for example, contain quite different numbers of atoms, because the atomic mass of platinum is much higher than that of magnesium.
How is a mole related to the atomic mass?
The atomic mass, in grams, is the mass of one mole of atoms.
Is avogadro's number the same as molar mass?
no youre thinking of molar mass and atomic weight although you use avogadro's number to find molar mass
How is the atomic mass for chlorine related to isotopes for that atom?
The average atomic mass is weighted by the most common isotopes and their relative abundance.
How many atoms in 1000 g of carbon?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.1000 grams C / (12.0 grams) × (6.02 × 1023 atoms) = 5.02 × 1025 atoms
How many atoms of sulfur are in 3.86 g?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.3.86 grams S / (32.1 grams) × (6.02 × 1023 atoms) = 7.24 × 1022 atoms
What is Avogadro constant?
Avogadro constant or number is the number of atoms in one mole, which is equal to 6.0221415 × 10^23. Edited to: The Avogadro constant is the number of particles (atoms, molecules or compounds) in one mole of a substance. It is the number of atoms in exactly 12g of carbon-12. As for all other elements, one mole of those is found in the relative atomic mass of that substance which is calculated relative to one twelfth of a carbon-12 atom e.g. one mole of oxygen atoms is in 16g of oxygen... and a mole was experiemtally worked out to contain 6.0221415 × 10^23 particles.
What were Avogadro's contributions to science?
He proposed in 1811, his famous hypothesis, now known as Avogadro's Law. The law stated that equal volumes of all gases at the same temperature and pressure contain the same number of molecules. His law helped to overcome John Dalton's atomic theory. Avogadro also distinguished between an atom and a molecule, to determine a table of atomic weights. Correction and standardization of atomic weights began in 1858, when Stanislao Cannizzaro, an Italian chemist, reminded other chemists about Avogadro's work.
Avogadro's number of p atoms wold have a mass of what?
30.97 or 31 grams The answer is the atomic weight
What is the mass of 5.0g of Fe how many atoms are present?
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.5.0 grams Fe / (55.9 grams) × (6.02 × 1023 atoms) = 5.38 × 1022 atoms
Which atomic mass number is closest to the average atomic mass of chlorine?
The periodic table is listed by atomic number which is highly related to atomic mass. Therefore the close ones would be to the left (Sulfur) and right(Argon). Sulfur is closest with an average distance of about 3.5 AMU.
