Answer:
The molar mass (Mm) of the compound is 127.39 g/mole
Explanation:
ΔT = Kf. molality
ΔT = change in temperature = Tfinal - Tinitial = 2.8 - 5.5
Kf = freezing point depression constant = - 4.3 C/m (always negative because temperature is decreasing)
molality = moles of solute/Kg of solvent = mole (n)/(20 x 10^-3 Kg of benzene)
(2.8 - 5.5) = (-4.3) x molality
molality = 0.6279 mole/kg
0.6279 = mole of compound/(20 x 10^-3)
mole of compound = 0.01256 mole
mole (n) = mass (m) divided by Molar mass (Mm)
Molar mass = mass of compound / mole of compound
m/n = 1.6/0.01256 = 127.39 g/mole
When uranium<span> comes in contact with oxygen in the air, it rusts, just like iron does, but </span>uranium<span> rust is black and not red. Like other heavy </span>atoms <span>such as iron, </span>uranium atoms<span> have more neutrons than they do protons. Not all </span>uranium atoms<span> have the </span>same<span> number of neutrons.</span>
