Answer :
To find the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, we need to understand a few key concepts:
1. Atomic Mass Unit (amu): The atomic mass of an element is typically given in atomic mass units (amu), but it also represents the mass of one mole of that element in grams. For potassium, the atomic mass is 39.1 amu, which means that one mole of potassium atoms has a mass of 39.1 grams.
2. Avogadro's Number: [tex]\(6.02 \times 10^{23}\)[/tex] atoms of any element is defined as one mole of that element. This is known as Avogadro's number.
Given these two points, if we have [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, we have exactly one mole of potassium.
Since one mole of potassium weighs 39.1 grams, the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms (one mole) of potassium is 39.1 grams.
Therefore, the correct answer is:
B. [tex]\(39.1 \text{ g}\)[/tex]
1. Atomic Mass Unit (amu): The atomic mass of an element is typically given in atomic mass units (amu), but it also represents the mass of one mole of that element in grams. For potassium, the atomic mass is 39.1 amu, which means that one mole of potassium atoms has a mass of 39.1 grams.
2. Avogadro's Number: [tex]\(6.02 \times 10^{23}\)[/tex] atoms of any element is defined as one mole of that element. This is known as Avogadro's number.
Given these two points, if we have [tex]\(6.02 \times 10^{23}\)[/tex] atoms of potassium, we have exactly one mole of potassium.
Since one mole of potassium weighs 39.1 grams, the mass of [tex]\(6.02 \times 10^{23}\)[/tex] atoms (one mole) of potassium is 39.1 grams.
Therefore, the correct answer is:
B. [tex]\(39.1 \text{ g}\)[/tex]
