https://file.aiquickdraw.com/mathbot/file/17303970210336md2vyyx.jpg

The question asks: "Which would have more atoms?"

To answer, we need to understand that 1 mole of any element contains the same number of atoms, given by Avogadro's number, which is approximately \(6.022 \times 10^{23}\) atoms. This constant applies universally to any substance in 1 mole.

- **1 mole of Lithium (Li)**: \(6.022 \times 10^{23}\) atoms
- **1 mole of Silicon (Si)**: \(6.022 \times 10^{23}\) atoms
- **1 mole of Cobalt (Co)**: \(6.022 \times 10^{23}\) atoms

Since each of these quantities represents 1 mole, they all contain the same number of atoms. Therefore, **none of them has more atoms than the others**.

### Answer: 
The correct answer is **D) None of the above**.

Would you like additional details, or do you have any other questions?

Here are some related questions for further exploration:
1. What is Avogadro's number and why is it important in chemistry?
2. How is the mole concept applied in chemical reactions?
3. How do different atomic masses affect the weight of 1 mole of different substances?
4. What is the difference between moles and molarity in chemistry?
5. How do you calculate the number of moles from a given mass of a substance?

**Tip:** Remember, the mole concept simplifies counting at the atomic level by allowing us to use macroscopic amounts to represent huge numbers of particles.

Which would have more atoms?
A) 1 mole of Lithium (Li)
B) 1 mole of Silicon (Si)
C) 1 mole of Cobalt (Co)
D) None of the above

Explore which of these elements—Lithium, Silicon, or Cobalt—contains more atoms in 1 mole. This problem uses the mole concept and Avogadro's number to show that each has the same number of atoms in a mole. Ideal for high school students in Grades 9-12.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation