Understanding Equivalent Weight
Equivalent weight of a metal can be defined as the mass of the metal that combines with or displaces 1 mole of hydrogen (or 8 grams of oxygen). The equivalent weight can be calculated using the formula:
Equivalent Weight = Atomic Mass / n
where 'n' is the valency of the metal.
Given Data
- Equivalent weights of the metal in two compounds:
- Compound 1: 18.6
- Compound 2: 28
Calculating Atomic Mass
To find the atomic mass of the metal, we need to determine 'n' for both compounds.
- For the first compound:
- Let n1 be the valency for the first compound.
- Hence, Atomic Mass = 18.6 * n1
- For the second compound:
- Let n2 be the valency for the second compound.
- Hence, Atomic Mass = 28 * n2
Equating the Atomic Mass
Since both expressions represent the atomic mass of the same metal, we can set them equal to each other:
18.6 * n1 = 28 * n2
From the above equation, we can explore possible integer values for n1 and n2 that make the equation valid.
Finding Possible Values
- If we assume n1 = 2 (common for metals), then:
- Atomic Mass = 18.6 * 2 = 37.2
- If n2 = 1, then:
- Atomic Mass = 28 * 1 = 28
This does not give a consistent value.
- Testing n1 = 1, n2 = 1:
- Atomic Mass = 18.6 * 1 = 18.6
- Atomic Mass = 28 * 1 = 28
Both do not yield an integer solution.
Testing Other Values
Through trial with other integers, we find that:
- n1 = 3 and n2 = 2 leads to:
- Atomic Mass = 18.6 * 3 = 55.8 (close to 56)
- Atomic Mass = 28 * 2 = 56
Conclusion
Thus, the atomic mass of the metal is approximately 56, making option 4) 56 the correct answer.