upon fully dissolving 2g of a metal in sulfuric acid6.8g of the metal sulphate is formed. The equivalent weight of the metal is
To find the equivalent weight of the metal, we first need to determine the number of equivalents of metal that reacted.
The equation for the reaction of the metal (M) with sulfuric acid (H2SO4) can be written as follows:
M + H2SO4 → MSO4 + H2
From the given information, we know that 2g of the metal fully dissolves and reacts with sulfuric acid to form 6.8g of the metal sulfate (MSO4).
Now, we need to find the number of moles of metal sulfate produced. We can do this by dividing the mass of the metal sulfate by its molar mass. The molar mass of metal sulfate can be calculated by adding the molar masses of the metal and the sulfate ion (SO4^2-).
The molar mass of sulfuric acid (H2SO4) is:
2(1g/mol of H) + 32g/mol of S + 4(16g/mol of O) = 98g/mol
Since we know that the metal sulfate (MSO4) is formed from the reaction of 2g of metal, we subtract the molar mass of sulfuric acid (98g/mol) from the mass of the metal sulfate (6.8g). This gives us the mass of the metal (M) in the metal sulfate:
Mass of metal (M) = Mass of metal sulfate - Mass of sulfuric acid
Mass of metal (M) = 6.8g - 2g = 4.8g
Now we can calculate the moles of metal (M) using its molar mass. Let's assume the molar mass of the metal (M) is "x" g/mol.
Moles of metal (M) = Mass of metal (M) / Molar mass of metal (M)
Moles of metal (M) = 4.8g / x g/mol
Since the reaction is a 1:1 ratio of metal to metal sulfate, the number of moles of metal is equal to the number of moles of metal sulfate. Therefore, we can write:
Moles of metal sulfate = Moles of metal (M) = 4.8g / x g/mol
Finally, to find the equivalent weight of the metal, we divide the mass of the metal by the number of equivalents:
Equivalent weight of metal = Mass of metal (M) / Moles of metal (M) = 4.8g / (4.8g / x g/mol) = x g/mol
Therefore, the equivalent weight of the metal is x g/mol.