A sacrificial anode used to protect a boat's hull from corrosion is made from 45.0 cm345.0\text{ cm}^345.0 cm3 of pure zinc. The density of zinc is 7.14 g/cm37.14\text{ g/cm}^37.14 g/cm3. Calculate the mass of the zinc anode.
Use the equation:
density=massvolume \text{density} = \frac{\text{mass}}{\text{volume}} density=volumemass53 exam-style questions on AQA GCSE Chemistry 3.1 Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations, covering 3.1.1 Conservation of mass and balanced chemical equations, 3.1.2 Relative formula mass, 3.1.3 Mass changes when a reactant or product is a gas, and 3.1.4 Chemical measurements. Each one has a worked solution and a mark scheme showing where the marks go.