A metal M of equivalent mass E forms an oxide of molecular formula MxO...
Explanation of the Atomic Mass of a Metal M
Introduction
Metal M has an equivalent mass E and forms an oxide of molecular formula MxOy. The equation that represents the atomic mass of the metal is given as:
(a) 2E(y/x)
(b) xyE
(c) E/y
Explanation of the Equation
The correct equation that represents the atomic mass of the metal M is (a) 2E(y/x). This equation is derived from the law of definite proportions, which states that the ratio of the masses of two elements in a compound is always constant.
In this case, we know that the molecular formula of the oxide is MxOy, which means that for every y moles of oxygen, there are x moles of the metal M.
We also know that the equivalent mass of the metal M is E, which means that one mole of the metal reacts with one mole of a monovalent acid or base.
Using this information, we can set up the following equation:
E/x = atomic mass of M
We also know that the molecular weight of the oxide is MxOy, which can be expressed as:
Mx + Oy = MxOy
We can find the molecular weight of the oxide by adding the atomic weights of M and O multiplied by their respective subscripts:
Mx + 16y = MxOy
Simplifying this equation, we get:
M = 16y/x + E
Substituting the value of E/x from the first equation, we get:
M = 16y/x + E/x
Multiplying both sides by x, we get:
Mx = 16y + Ex
Dividing both sides by y, we get:
Mx/y = 16 + E/y
Substituting the value of x/y, we get:
M = 2E(y/x)
Therefore, the correct equation that represents the atomic mass of the metal M is (a) 2E(y/x).
Conclusion
In conclusion, the atomic mass of a metal M that forms an oxide of molecular formula MxOy is represented by the equation (a) 2E(y/x). This equation is derived from the law of definite proportions and takes into account the equivalent mass of the metal and the molecular weight of the oxide.