To answer this question, we need to rely on our knowledge of moles, Avogadro's number, and the concept of molar mass.
### First Statement:
"There are [tex]\(6.022 \times 10^{23}\)[/tex] atoms of carbon in one mole of carbon."
This statement is true because Avogadro's number, which is [tex]\(6.022 \times 10^{23}\)[/tex], defines the number of constituent particles (atoms, molecules, etc.) in one mole of a given substance.
### Second Statement:
"There is 1 mol of sodium atoms in one gram of sodium."
This statement is false. The molar mass of sodium (Na) is approximately 23 grams per mole. Therefore, one gram of sodium corresponds to [tex]\(\frac{1}{23}\)[/tex] moles of sodium atoms, not 1 mole.
### Third Statement:
"There are [tex]\(6.022 \times 10^{23}\)[/tex] molecules of ammonia in one mole of ammonia."
This statement is true. Similar to the first statement, by definition of Avogadro's number, one mole of any substance contains exactly [tex]\(6.022 \times 10^{23}\)[/tex] constituent particles—in this case, molecules of ammonia (NH[tex]\(_3\)[/tex]).
### Fourth Statement:
"The number of atoms in a balloon with 1 mol of helium is equal to Avogadro's number."
This statement is true. One mole of helium (He), like any other element, contains [tex]\(6.022 \times 10^{23}\)[/tex] atoms, as it adheres to Avogadro's law.
So, summarizing the correctness of each statement:
- True: There are [tex]\(6.022 \times 10^{23}\)[/tex] atoms of carbon in one mole of carbon.
- False: There is 1 mol of sodium atoms in one gram of sodium.
- True: There are [tex]\(6.022 \times 10^{23}\)[/tex] molecules of ammonia in one mole of ammonia.
- True: The number of atoms in a balloon with 1 mol of helium is equal to Avogadro's number.
The true statements are:
1. There are [tex]\(6.022 \times 10^{23}\)[/tex] atoms of carbon in one mole of carbon.
3. There are [tex]\(6.022 \times 10^{23}\)[/tex] molecules of ammonia in one mole of ammonia.
4. The number of atoms in a balloon with 1 mol of helium is equal to Avogadro's number.
