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

Volume = 15.46-11.00mL = 4.46mL

Density = mass/vol = 18.592g/4.46mL = 4.1686g/mL = 4.1686g/cm^3

Answer 2

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.

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

$\text{Density of metal}=\frac{17.676g}{4.46mL}=3.963g/mL$

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