Question

The density of water changes at different temperatures, most dramatically as it undergoes freezing to produce ice. You have an ice cube with a volume of 75.0 mL in a cup at a temperature of -1°C where its density is 0.9168 g/mL. You melt the ice cube by raising the temperature to 25.00 °C, where the density of liquid water is 0.9970 g/mL. What volume does the water now occupy?

Answer 1

The volume occupied by the water at 25°C, after melting the ice cube, is 68.97 mL. This is calculated by first finding the mass of the ice using its density at -1°C, and then using the mass with the density of water at 25°C to find the new volume.

Step-by-step explanation:

The task involves understanding the density of water and its changes with temperature to determine the volume occupied by melted ice. When the ice cube melts, the mass of water remains the same, but the density changes, which leads to a change in volume. We can calculate the mass of the ice cube using its initial volume and density, and then use the density of water at 25°C to find the new volume.

First, let's calculate the mass of the ice at -1°C using the given density:

Mass = density × volume = 0.9168 g/mL × 75.0 mL = 68.76 g

Since mass is conserved during melting, the mass of the liquid water is also 68.76 g. Now, we can calculate the new volume using the density of water at 25°C:

Volume = mass / density = 68.76 g / 0.9970 g/mL = 68.97 mL

Therefore, the volume occupied by the water at 25°C is 68.97 mL.