Question
Metal Density (g/cm3)
aluminum 2.70
zinc 7.14
iron 7.87
copper 8.96
silver 10.49
lead 11.34
mercury 13.55
gold 19.32
25
What is the identity of a sample that has a mass of 2.44 g and a volume of 0.34 cm3?
A.
gold
B.
aluminum
C.
zinc
D.
copper
Answers
GPT-4o mini
To determine the identity of the sample, we can calculate its density using the formula:
\[
\text{Density} = \frac{\text{Mass}}{\text{Volume}}
\]
Given:
- Mass = 2.44 g
- Volume = 0.34 cm³
Let's calculate the density:
\[
\text{Density} = \frac{2.44 \, \text{g}}{0.34 \, \text{cm}^3} \approx 7.18 \, \text{g/cm}^3
\]
Now, we can compare this density with the densities of the metals provided:
- Aluminum: 2.70 g/cm³
- Zinc: 7.14 g/cm³
- Iron: 7.87 g/cm³
- Copper: 8.96 g/cm³
- Silver: 10.49 g/cm³
- Lead: 11.34 g/cm³
- Mercury: 13.55 g/cm³
- Gold: 19.32 g/cm³
The calculated density of approximately 7.18 g/cm³ is closest to the density of zinc (7.14 g/cm³).
Therefore, the identity of the sample is:
**C. zinc**
\[
\text{Density} = \frac{\text{Mass}}{\text{Volume}}
\]
Given:
- Mass = 2.44 g
- Volume = 0.34 cm³
Let's calculate the density:
\[
\text{Density} = \frac{2.44 \, \text{g}}{0.34 \, \text{cm}^3} \approx 7.18 \, \text{g/cm}^3
\]
Now, we can compare this density with the densities of the metals provided:
- Aluminum: 2.70 g/cm³
- Zinc: 7.14 g/cm³
- Iron: 7.87 g/cm³
- Copper: 8.96 g/cm³
- Silver: 10.49 g/cm³
- Lead: 11.34 g/cm³
- Mercury: 13.55 g/cm³
- Gold: 19.32 g/cm³
The calculated density of approximately 7.18 g/cm³ is closest to the density of zinc (7.14 g/cm³).
Therefore, the identity of the sample is:
**C. zinc**