Skip to main content
Ch.2 - Atoms & Elements
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.2 - Atoms & ElementsProblema 101
Capitolo 2, Problema 101

How many carbon atoms are there in a diamond (pure carbon) with a mass of 83 mg?

Guida verificata passo dopo passo
1
Convert the mass of the diamond from milligrams to grams by dividing by 1000, since there are 1000 milligrams in a gram.
Use the molar mass of carbon, which is approximately 12.01 g/mol, to convert the mass of the diamond in grams to moles of carbon. This is done by dividing the mass in grams by the molar mass of carbon.
Apply Avogadro's number, which is approximately \(6.022 \times 10^{23}\) atoms/mol, to convert the moles of carbon to the number of carbon atoms. Multiply the number of moles by Avogadro's number.
Ensure that all units cancel appropriately during the calculations to confirm that the final result is in atoms.
Review the steps to ensure that each conversion is correctly applied and that the logical flow from mass to moles to atoms is clear.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
1m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Molar Mass of Carbon

The molar mass of carbon is approximately 12.01 g/mol. This value represents the mass of one mole of carbon atoms, which is essential for converting between mass and the number of atoms. In this question, knowing the molar mass allows us to calculate how many moles of carbon are present in the given mass of diamond.
Video consigliato:
Percorso guidato
02:11
Molar Mass Concept

Avogadro's Number

Avogadro's number, approximately 6.022 x 10²³, is the number of atoms, ions, or molecules in one mole of a substance. This constant is crucial for determining the number of individual carbon atoms in the diamond once the number of moles is calculated from the mass. It provides a bridge between the macroscopic scale of grams and the microscopic scale of atoms.
Video consigliato:
Percorso guidato
02:11
Avogadro's Law

Mass to Moles Conversion

To find the number of carbon atoms in a diamond sample, we first convert the mass of the sample (in grams) to moles using the formula: moles = mass (g) / molar mass (g/mol). This conversion is fundamental in stoichiometry, allowing us to relate the mass of a substance to the number of particles it contains, which is necessary for answering the question.
Video consigliato:
Percorso guidato
02:28
Mass and Moles Conversion
Pratica correlata
Domanda del libro di testo

Calculate the mass, in grams, of each sample. c. 1.8×1023 lead atoms

739
views
Domanda del libro di testo

Using scanning tunneling microscopy, scientists at IBM wrote the initials of their company with 35 individual xenon atoms (as shown below). Calculate the total mass of these letters in grams.

413
views
Domanda del libro di testo

Calculate the average mass, in grams, of one platinum atom.

1331
views
Domanda del libro di testo

How many helium atoms are there in a helium blimp containing 587 kg of helium?

Domanda del libro di testo

Calculate the mass, in grams, of each sample. d. 7.9×1021 uranium atoms

1340
views
Domanda del libro di testo

Calculate the mass, in kg, of each sample. a. 7.55×1026 cadmium atoms b. 8.15×1027 nickel atoms c. 1.22×1027 manganese atoms d. 5.48×1029 lithium atoms

1184
views
1
comments