Answer :
To find the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, we need to use the relationship between atomic mass and Avogadro's number. Here's a step-by-step solution:
1. Understand the Concept:
- The atomic mass of potassium is given as 39.1 atomic mass units (amu).
- Avogadro’s number ([tex]\(6.022 \times 10^{23}\)[/tex]) indicates the number of atoms in one mole of any substance.
- The atomic mass in amu is numerically equal to the mass of one mole of atoms in grams.
2. Relate Atomic Mass to Mass in Grams:
- Since the atomic mass of potassium is 39.1 amu, this means one mole (i.e., [tex]\(6.022 \times 10^{23}\)[/tex] atoms) of potassium has a mass of 39.1 grams.
3. Apply the Concept:
- Given [tex]\(6.02 \times 10^{23}\)[/tex] atoms, which is approximately one mole, the mass of these atoms in grams will be the same as the atomic mass in grams.
4. Conclusion:
- Therefore, the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium is 39.1 grams.
So, the correct answer is:
B. [tex]\(39.1\)[/tex] (which represents grams).
1. Understand the Concept:
- The atomic mass of potassium is given as 39.1 atomic mass units (amu).
- Avogadro’s number ([tex]\(6.022 \times 10^{23}\)[/tex]) indicates the number of atoms in one mole of any substance.
- The atomic mass in amu is numerically equal to the mass of one mole of atoms in grams.
2. Relate Atomic Mass to Mass in Grams:
- Since the atomic mass of potassium is 39.1 amu, this means one mole (i.e., [tex]\(6.022 \times 10^{23}\)[/tex] atoms) of potassium has a mass of 39.1 grams.
3. Apply the Concept:
- Given [tex]\(6.02 \times 10^{23}\)[/tex] atoms, which is approximately one mole, the mass of these atoms in grams will be the same as the atomic mass in grams.
4. Conclusion:
- Therefore, the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium is 39.1 grams.
So, the correct answer is:
B. [tex]\(39.1\)[/tex] (which represents grams).
