Thank you for visiting Select the correct answer The atomic mass of potassium is 39 1 What is the mass of tex 6 02 times 10 23 tex atoms. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!
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]
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