🤓 Based on our data, we think this question is relevant for Professor Browning, Wilson & De Backere's class at TORONTO.

We have to determine if the found bracelet if made of silver or not.

We have the density of silver metal, 10.5 g/cm^{3}. We will *calculate the density of the bracelet and compare it with the density of silver* to determine if the bracelet is made from silver metal.

**The formula for density is:**

$\overline{){\mathbf{density}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{mass}}{\mathbf{volume}}}$

You are beachcombing on summer vacation and find a silver bracelet. You take it to the jeweler and he tells you that it is silver plated and will give you $10 for it. You do not want to be swindled so you take the bracelet to your chemistry lab and find its mass on a balance (80.0 g). To measure the volume you place the bracelet in a graduated cylinder, containing 10.0 mL of water at 20 ^{o}C. The final volume in the graduated cylinder after the bracelet has been added is 17.61 mL. The density of silver at 20 ^{o}C is 10.5 g/cm^{3} and 1 cm^{3}= 1 mL.

What can you conclude about the identity of the metal in the bracelet?