Boiling-point elevation is a colligative property.
That means, the the boiling-point elevation depends on the molar content (fraction) of solute.
The dependency is ΔTb = Kb*m
Where ΔTb is the elevation in the boiling point, kb is the boiling constant, and m is the molality.
A solution of 6.00 g of Ca(NO3) in 30.0 g of water has 4 times the molal concentration of a solution of 3.00 g of Ca(NO3)2 in 60.0 g of water.:
(6.00g/molar mass) / 0.030kg = 200 /molar mass
(3.00g/molar mass) / 0.060kg = 50/molar mass
=> 200 / 50 = 4.
Then, given the direct proportion of the elevation of the boiling point with the molal concentration, the solution of 6.00 g of CaNO3 in 30 g of water will exhibit a greater boiling point elevation.
Or, what is the same, the solution with higher molality will have the higher boiling point.
I think the correct answer from the choices listed above is the first option. Compared to compounds that possess only dipole-dipole intermolecular forces, compounds that possess hydrogen bonding generally have <span>higher melting points. This is because hydrogen bonding is a stronger force than dipole-dipole.</span>
The main difference between the 3 isotopes of hydrogen are the number of neutrons in the nucleus. Hydrogen has no neutrons, Deuterium has one neutron, and tritium has two neutrons. All three have one proton and one electron.
NO2- +7H+ + 6e->> NH3 + 2H2O ( N goes from +3 to -3)
<span>Al + 2 H2O >> AlO2- + 4H+ + 3e- </span>
<span>NO2- + 2Al + 2H2O >> NH3 + 2AlO2- + H+ </span>
<span>add OH- on the left and on the right </span>
<span>NO2- + 2 Al + H2O + OH- >> NH3 + 2 AlO2-</span>
Carbon is found in all four.