Chapter 8, Problem 1CE

Interpretation Introduction

(a)

Interpretation:

The mass of $1$ atom of carbon is to be stated.

Concept introduction:

The atomic mass of an atom is the amount of matter present in the atom of an element. It is the multiple of $1/{12}^{\text{th}}$ mass of the $\text{carbon-}12$ atom. It is expressed in $\text{amu}$ where $1\text{amu}=1.66\times {10}^{-23}\text{g}$. Avogadro’s number is represented by symbol $\text{N}$. It is the number of units: atoms, electrons, molecules, or ions present in one mole of a substance. The value of $\text{N}$ is $6.022\times {10}^{23}$.

Answer to Problem 1CE

The mass of $1$ atom of carbon is $12.01\text{amu}$.

Explanation of Solution

The atomic mass of an atom is the amount of matter present in the atom of an element. It is the multiple of $1/{12}^{\text{th}}$ mass of the $\text{carbon-}12$ atom. It is expressed in amu where $1\text{amu}=1.66\times {10}^{-23}\text{g}$.

The mass of an atom of carbon is $12.01\text{amu}$.

Conclusion

The mass of $1$ atom of carbon is found to be $12.01\text{amu}$.

Interpretation Introduction

(b)

Interpretation:

The mass of $6.022\times {10}^{23}$ atoms of carbon is to be stated.

Concept introduction:

The atomic mass of an atom is the amount of matter present in the atom of an element. It is the multiple of $1/{12}^{\text{th}}$ mass of the $\text{carbon-}12$ atom. It is expressed in $\text{amu}$ where $1\text{amu}=1.66\times {10}^{-23}\text{g}$. Avogadro’s number is represented by symbol $\text{N}$. It is the number of units: atoms, electrons, molecules, or ions present in one mole of a substance. The value of $\text{N}$ is $6.022\times {10}^{23}$.

Answer to Problem 1CE

The Avogadro number of carbon has a mass of $12.01\text{g}$.

Explanation of Solution

Avogadro’s number is the number of units: atoms, electrons, molecules, or ions present in one mole of a substance. It is represented by symbol $\text{N}$. The value of $\text{N}$ is $6.022\times {10}^{23}$.

Therefore, $6.022\times {10}^{23}$ atoms of carbon is equal to the mass of one carbon atom, that is, $12.01\text{g}$.

Conclusion

The mass of $6.022\times {10}^{23}$ atoms of carbon is $12.01\text{g}$.