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Ch.3 - Molecules, Compounds & Chemical Equations
Chapter 3, Problem 62

What is the mass of each sample? a. 15.7 mol HNO3 b. 1.04 × 10^-3 mol H2O2 c. 72.1 mmol SO2 d. 1.23 mol xenon difluoride

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all the atoms in a molecule. For example, the molar mass of HNO3 is approximately 63.01 g/mol, which is essential for converting moles to grams.
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Molar Mass Concept

Conversion Between Moles and Mass

To find the mass of a substance from its amount in moles, the formula used is: mass (g) = moles × molar mass (g/mol). This relationship allows chemists to convert between the number of moles of a substance and its corresponding mass, facilitating calculations in stoichiometry and chemical reactions.
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Mass and Moles Conversion

Unit Conversions

Unit conversions are necessary when dealing with different units of measurement, such as converting millimoles (mmol) to moles (mol). Since 1 mmol is equal to 0.001 mol, understanding these conversions is crucial for accurately calculating the mass of substances in various units, ensuring consistency in chemical calculations.
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Conversion Factors