What is the mass, in grams, of each elemental sample? c. 1.75×10-3 mol Hg

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Identify the molar mass of mercury (Hg) from the periodic table. The molar mass of Hg is approximately 200.59 g/mol.

Use the formula: \( \text{mass} = \text{moles} \times \text{molar mass} \) to find the mass of the sample.

Substitute the given number of moles (1.75 \times 10^{-3} \text{ mol}) and the molar mass of Hg (200.59 g/mol) into the formula.

Calculate the product of the moles and the molar mass to find the mass in grams.

Ensure the units are consistent and the final answer is expressed in grams.

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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 a crucial concept in stoichiometry, as it allows for the conversion between the number of moles of a substance and its mass. For example, the molar mass of mercury (Hg) is approximately 200.59 g/mol, which means one mole of mercury weighs 200.59 grams.

Moles

A mole is a unit in chemistry that represents a specific quantity of particles, typically atoms or molecules. One mole is defined as 6.022 × 10²³ particles, known as Avogadro's number. Understanding moles is essential for quantifying substances in chemical reactions and for converting between mass and number of particles.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It involves calculations that use the molar mass and the concept of moles to determine how much of each substance is involved in a reaction. In this context, stoichiometry helps in calculating the mass of elemental samples from the given number of moles.