Question

A piece of metal (mass = 17.676 g) is placed in 11.00 mL of chloroform (d = 1.498 g/mL) in a 25-mL graduated cylinder. The chloroform level increases to 15.46 mL. The best value for density of this metal from these data is

Answer 1

Answer : The density of metal will be 3.963 g/mL

Explanation : Given,

Mass of metal = 17.676 g

Initial volume of chloroform = 11.00 mL

Final volume of chloroform = 15.46 mL

First we have to calculate the volume of metal.

Volume of metal = Final volume of chloroform - Initial volume of chloroform

Volume of metal = 15.46 - 11.00 = 4.46 mL

Now we have to calculate the density of metal.

`\text{Density of metal}=\frac{\text{Mass of metal}}{\text{Volume of metal}}`

`\text{Density of metal}=(17.676g)/(4.46mL)=3.963g/mL`

Therefore, the density of metal will be 3.963 g/mL