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Chapter 3: Problem 28

If the mass of a gold atom is 196.97 amu, what is the atom's molar mass?

Short Answer

Expert verified
The molar mass of a gold atom is 196.97 g/mol.

Step by step solution

01

Understand the relation between amu and g/mol.

In chemistry, it is important to note that the atomic mass of an element, expressed in atomic mass units (amu), is numerically the same as the molar mass of the element, expressed in grams/mol. For example, the atomic mass of carbon-12 is 12 amu and the molar mass of carbon-12 is 12 g/mol.
02

Convert atomic mass to molar mass

Since the molar mass and atomic mass are numerically the same but in different units, to find the molar mass of a gold atom, simply change the units. From the problem, we know that a gold atom has a mass of 196.97 amu. Therefore, the molar mass of a gold atom is 196.97 g/mol.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Mass
The concept of atomic mass is foundational in understanding chemistry and how elements interact. Atomic mass is the weight of an atom expressed in atomic mass units (amu). It represents the average mass of the atoms of an element, calculated using the relative abundance of isotopes in a naturally occurring element. To make it digestible:
  • Each element has isotopes, which are atoms with differing numbers of neutrons.
  • The atomic mass takes these isotopes into account, providing a weighted average.
  • It's a crucial number that helps scientists understand how much of an element's atoms exist in a sample.
By knowing the atomic mass of an element, we can deduce other important chemical properties and behaviors.
Atomic Mass Units (amu)
Atomic mass units, abbreviated as amu, are the standard unit of measurement used for expressing atomic mass. Since atoms are extremely small, amu provides a manageable way to measure their mass. One amu is defined as one twelfth of the mass of a carbon-12 atom, which is approximately equal to the mass of a single proton or neutron.
For students to grasp the use of amu:
  • It allows us to express tiny masses in a comprehensible way.
  • Ensures consistency and precision across scientific measurements.
  • Forms the basis for calculating molar masses.
Understanding amu is vital for performing accurate chemistry calculations and bridging the microscopic atomic scale to macroscopic quantities.
Chemistry Calculations
Chemistry calculations often involve transitioning between the microscopic world of atoms and the macroscopic world of measurable substances. When dealing with substances in chemistry, calculations involving molar mass become crucial. The molar mass of an element or compound is the mass of one mole of that substance, typically expressed in grams per mole (g/mol).
Here's how chemistry calculations tie the concepts together:
  • Atomic mass in amu directly translates to molar mass in g/mol, facilitating calculations in the lab.
  • Knowing this helps in stoichiometry, which involves calculating relationships between reactants and products in chemical reactions.
  • Proper chemistry calculations ensure accurate experimental results and help in quantifying materials accurately.
Thus, understanding chemistry calculations transforms theoretical knowledge into practical laboratory skills.

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