Chapter 2: Problem 109
A cube made of platinum (Pt) has an edge length of \(1.0 \mathrm{~cm} .\) (a) Calculate the number of \(\mathrm{Pt}\) atoms in the cube. (b) Atoms are spherical in shape. Therefore, the \(\mathrm{Pt}\) atoms in the cube cannot fill all of the available space. If only 74 percent of the space inside the cube is taken up by Pt atoms, calculate the radius in picometers of a \(\mathrm{Pt}\) atom. The density of \(\mathrm{Pt}\) is \(21.45 \mathrm{~g} / \mathrm{cm}^{3}\) and the mass of a single \(\mathrm{Pt}\) atom is \(3.240 \times 10^{-22} \mathrm{~g}\). [The volume of a sphere of radius \(r\) is \(\left.(4 / 3) \pi r^{3} .\right]\)
Short Answer
Step by step solution
Key Concepts
These are the key concepts you need to understand to accurately answer the question.