Answer :
To find the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, you'll need to understand how atomic mass and Avogadro's number work together.
1. Understand Atomic Mass: The atomic mass of potassium is given as 39.1 grams per mole. This means that one mole of potassium atoms, which is [tex]\(6.02 \times 10^{23}\)[/tex] atoms (Avogadro's number), weighs 39.1 grams.
2. Relate Atoms to Moles: When you're asked for the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, you're essentially being asked for the mass of one mole of potassium atoms. This is because [tex]\(6.02 \times 10^{23}\)[/tex] atoms is the definition of a mole.
3. Calculate the Mass: Since one mole of potassium atoms has a mass of 39.1 grams, and the problem asks for the mass of exactly one mole of potassium ([tex]\(6.02 \times 10^{23}\)[/tex] atoms), the answer is just the atomic mass expressed in grams.
Therefore, the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium is 39.1 grams.
The answer is:
B. 39.1 g
1. Understand Atomic Mass: The atomic mass of potassium is given as 39.1 grams per mole. This means that one mole of potassium atoms, which is [tex]\(6.02 \times 10^{23}\)[/tex] atoms (Avogadro's number), weighs 39.1 grams.
2. Relate Atoms to Moles: When you're asked for the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, you're essentially being asked for the mass of one mole of potassium atoms. This is because [tex]\(6.02 \times 10^{23}\)[/tex] atoms is the definition of a mole.
3. Calculate the Mass: Since one mole of potassium atoms has a mass of 39.1 grams, and the problem asks for the mass of exactly one mole of potassium ([tex]\(6.02 \times 10^{23}\)[/tex] atoms), the answer is just the atomic mass expressed in grams.
Therefore, the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium is 39.1 grams.
The answer is:
B. 39.1 g
