Final answer:
To convert 1.5 × 10²³ lead atoms to grams, the molar mass of lead and Avogadro's number are used to calculate the mass, which is approximately 51.8 g. When rounded to two significant figures, the result is 52 g, and the provided answer choices do not include the correct answer.
Step-by-step explanation:
To convert 1.5 × 10²³ lead atoms to grams, we use the concept of molar mass. The molar mass of lead (Pb) is 207.2 g/mol. We know that one mole of any substance contains Avogadro's number of particles, which is approximately 6.022 × 10²³ particles/mol. Therefore, to find the mass in grams of 1.5 × 10²³ lead atoms, we can set up a proportion where:
mass of 1.5 × 10²³ atoms / 1.5 × 10²³ = 207.2 g / 6.022 × 10²³
By cross-multiplying and solving for the mass of the lead atoms, we get:
mass = (1.5 × 10²³ × 207.2 g) / (6.022 × 10²³)
mass ≈ 51.8 g
When rounded to two significant figures, the mass of the lead atoms is 52 g. So, none of the provided answer choices (207 g, 41 g, 26 g, 31 g) are correct.