In each of the following groups of substances, pick the one that has the given property, respectively:
I. lowest boiling point: HBr, Kr, Br2
II. highest freezing point: H2O, LiBr, HF
III. lowest vapor pressure at 25°C: Cl2, Br2, I2, At2
IV. lowest freezing point: H2, CO, CO2
PLEASE EXPLAIN!!!!
I. lowest boiling point: HBr, Kr, Br2 --> must be the species with lowest intermolecular forces: Br2 = nonpolar Kr = nonpolar, HBr = polar
then between Kr and Br2
Br2 > mass than Kr, therefore lowest BP is Kr
II. highest freezing point: H2O, LiBr, HF --> the species with MOST interactions
from th elist, LiBr --> highest freezing ponit, since it is an ionic salt, has higher interactoins than any other molecular species
III. lowest vapor pressure at 25°C: Cl2, Br2, I2, At2
vapor pressure --> tendecy to become a vapor, therefore, the heavier the species, the lower vapor pressure
from the list, At has the lowest vapor pressure
IV. lowest freezing point: H2, CO, CO2 --> CO is polar, all other are nonpolar. For lowest freezing point, we need the least intermolecular forces
H2 has lowr mass than cO2, therefore, H2 has lowest freezing point
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