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?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Density of Non-Geometric Objects concept. You can view video lessons to learn Density of Non-Geometric Objects. Or if you need more Density of Non-Geometric Objects practice, you can also practice Density of Non-Geometric Objects practice problems.

What professor is this problem relevant for?

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