At room temperature, ethanol's density is 0.789 g/mL while water's density is 0.997 g/mL. When a few milliliters of ethanol are added to water, the two liquids mix. A student is given a unknown liquid at room temperature and experimentally determines its density to be 0.947 g/mL. Is the liquid is pure ethanol, pure water, or a mixture? If it is a mixture, does it contain more ethanol or more water?

To determine whether the unknown liquid is pure ethanol, pure water, or a mixture, we can compare its density to the densities of ethanol and water.

Given that the density of the unknown liquid is 0.947 g/mL, we can compare this value to the known densities of ethanol and water.

Since the density of ethanol is 0.789 g/mL and the density of water is 0.997 g/mL, we can infer the following:

- If the density of the unknown liquid is closer to 0.789 g/mL, then it is likely a mixture containing more ethanol.
- If the density of the unknown liquid is closer to 0.997 g/mL, then it is likely a mixture containing more water.

Let's compare the value of 0.947 g/mL to the densities of ethanol and water:

- The density of the unknown liquid (0.947 g/mL) is closer to the density of water (0.997 g/mL).

Based on this comparison, we can conclude that the unknown liquid is a mixture containing more water than ethanol.