A chemistry student is given 4.00 L of a clear aqueous solution at 22.。C. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 22.° C. The solution remains clear. He then evaporates all of the water under vacuum. A precipitate remains. The student washes, dries and weighs the precipitate. It weighs 0.56 kg. Using only the information above, can you calculate the solubility of X in water at 22.° C
If you said yes, calculate it
Be sure your answer has a unit symbol and 2 no .0 it. significant digits.

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

it is stable as it is in group 0 which have full outer shells of electrons