Chemists generally use the mole as the unit for the number of atoms or molecules of a material. One mole (abbreviated mol) is equal to 6.022×10 23 molecular entities (Avogadro’s number), and each element has a different molar mass depending on the weight of 6.022×10 23 of its atoms (1 mole). MHg2Br2 = mHg2Br2 nHg2Br2 = 560.98 g mol−1 M Hg 2 Br 2 = m Hg 2 Br 2 n Hg 2 Br 2 = 560.98 g mol − 1. The molar mass is numerically the same as the atomic or molecular weight, but it has units of grams per mole. The equation, which defines the molar mass, has the same form as those defining density, and the Avogadro constant.

An example of calculating the molar mass of an ideal gas: A scientist carries out an experiment to determine the molar mass of a 2.84-g sample of a colorless liquid which exerts 756 mmHg pressure when vaporized in a 260-mL flask at 142 o C. What is the molecular mass of this compound?

The chemical analysis of caffeine shows that it contains 49.18% carbon, 5.39% hydrogen, 28.65% nitrogen, and 16.68% oxygen by mass, and its experimentally determined molar mass is 196 g/mol. Given: percent composition and molar mass. Asked for: molecular formula. Strategy: Assume 100 g of caffeine. The numbers in a conversion factor come from the coefficients of the balanced chemical equation. The following six mole ratios can be written for the ammonia forming reaction above. 1mol N 23mol H 2 or 3molH 21molN 21mol N 22molNH 3 or 2mol NH 31molN 23mol H 22molNH 3 or 2mol NH 33molH 2. In a mole ratio problem, the given substance, expressed Molar Mass is the mass of one mole of a substance in grams/mole, while Molecular Mass is the sum of atomic masses of all atoms in a molecule in atomic mass units (amu). Key Differences Molar Mass is typically expressed in grams per mole (g/mol). TTBip.
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    • is molecular mass and molar mass the same