Chapter 3: Problem 20
How many protons are in (a) an atom of platinum? (b) one mole of platinum? (c) one gram of platinum?
Short Answer
Expert verified
Answer: There are 2.40 x 10^23 protons in one gram of platinum.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Avogadro's Number
Imagine a very large number that's crucial in the world of chemistry; this number is known as Avogadro's number, which is approximately equal to \(6.022 \times 10^{23}\). It's named after the Italian scientist Amedeo Avogadro and is the number of units in one mole of any substance.
Think of it as the bridge between the microscopic world of atoms and molecules and our everyday, macroscopic world. Just as a dozen always refers to 12 things, one mole always contains Avogadro's number of particles, whether those particles are atoms, ions, or molecules. This concept is at the heart of many calculations in chemistry, including determining the number of atoms or molecules in a given mass of a substance—like how many protons are in a mole of platinum.
Think of it as the bridge between the microscopic world of atoms and molecules and our everyday, macroscopic world. Just as a dozen always refers to 12 things, one mole always contains Avogadro's number of particles, whether those particles are atoms, ions, or molecules. This concept is at the heart of many calculations in chemistry, including determining the number of atoms or molecules in a given mass of a substance—like how many protons are in a mole of platinum.
Mole Concept
To understand the mole concept, it helps to think about buying eggs. An egg carton typically holds a dozen eggs. In chemistry, instead of counting items one by one, we count them by the 'carton,' except this carton is called a mole, and it's a lot bigger, containing Avogadro's number of items.
The mole is a standard unit of measurement used in chemistry to express amounts of a chemical substance. It allows chemists to work with the subatomic world with macroscopic amounts of material. When we talk about one mole of an element or compound, we're referring to exactly \(6.022 \times 10^{23}\) of their fundamental units (atoms, molecules, ions, etc.). For example, one mole of platinum contains \(6.022 \times 10^{23}\) platinum atoms.
The mole is a standard unit of measurement used in chemistry to express amounts of a chemical substance. It allows chemists to work with the subatomic world with macroscopic amounts of material. When we talk about one mole of an element or compound, we're referring to exactly \(6.022 \times 10^{23}\) of their fundamental units (atoms, molecules, ions, etc.). For example, one mole of platinum contains \(6.022 \times 10^{23}\) platinum atoms.
Molar Mass
Every chemist's toolbox includes the term 'molar mass', which represents the mass of one mole of a given substance. Expressed in grams per mole (g/mol), the molar mass is numerically equivalent to the atomic or molecular weight of a substance.
For instance, the molar mass of platinum is 195.08 g/mol, which means every mole of platinum has a mass of 195.08 grams. This concept is vitally important when converting between the number of moles and the mass of a substance. It provides a way to measure precise amounts of a substance in a lab by relating the mole (a count of particles) to mass (something we can measure on a scale).
For instance, the molar mass of platinum is 195.08 g/mol, which means every mole of platinum has a mass of 195.08 grams. This concept is vitally important when converting between the number of moles and the mass of a substance. It provides a way to measure precise amounts of a substance in a lab by relating the mole (a count of particles) to mass (something we can measure on a scale).
