Final answer:
To find the number of copper atoms in a copper sphere with a radius of 0.929 inches, calculate the volume of the sphere, convert it to mass using copper's density, then to moles using atomic mass, and finally multiply by Avogadro's number.
Step-by-step explanation:
To calculate the number of copper atoms in a sphere of pure copper with a radius of 0.929 inches, we first need to determine the volume of the sphere, and then use the copper's density along with Avogadro's number to find the total number of atoms. The volume of a sphere (V) is given by the formula V = 4/3 * π * r³, where r is the radius. Since 1 inch = 2.54 cm, we convert the radius into centimeters before calculating the volume.
Once the volume is found, we use the density of copper (8.95 g/cm³) to calculate the mass of copper in the sphere. This mass can be converted to moles by using the atomic mass of copper (63.54 g/mol), and finally, by using Avogadro's number (6.02 × 10²³ atoms/mol), we can find the number of copper atoms in the sphere.