To determine if the sample is really silver, we first need to calculate its density using the mass and volume provided. Density (\(d\)) is calculated using the formula:
\[ d = \frac{m}{V} \]
where \(m\) is the mass of the sample and \(V\) is the volume.
Given Data:
- Mass \(m = 1.7 , \text{kg}\)
- Volume \(V = 0.164 , \text{liters}\)
First, we need to convert the volume from liters to milliliters because the density of silver is given in kg/mL.
1 liter = 1000 mL, so:
\[ 0.164 , \text{liters} = 0.164 \times 1000 , \text{mL} = 164 , \text{mL} \]
Now we can calculate the density:
\[ d = \frac{1.7 , \text{kg}}{164 , \text{mL}} \approx 0.01037 , \text{kg/mL} \]
To make it easier to compare, let's convert this density to grams per milliliter since 1 kg = 1000 grams:
\[ d \approx 0.01037 , \text{kg/mL} \times 1000 , \text{g/kg} = 10.37 , \text{g/mL} \]
Comparison with Silver's Density:
The density of silver is approximately 10.49 g/mL.
Now, let's observe our calculated density of 10.37 g/mL. The density is very close to the known density of silver, but it is slightly lower.
Conclusion:
While the density of your sample (10.37 g/mL) is very close to that of silver (10.49 g/mL), it is slightly lower, which could indicate that it is not pure silver or that it may be an alloy or another metal. Further tests, such as chemical analysis or conductivity tests, may be needed to confirm the identity of the material.
2 answers