Choose the substance in each pair with the highest boiling point. CH_4 C_3H_s H_
ID: 1018030 • Letter: C
Question
Choose the substance in each pair with the highest boiling point. CH_4 C_3H_s H_2 O H_2 S CH_3 F CF_4 What factor, other than the delta H_solution determines whether an ionic compound will dissolve entropy enthalpy ion - dipole forces The hydrophobic effect is responsible for micelle formation by phospholipids Insolubility of oil in water folding of proteins in 3-dimensions all of these Consider the following solutions: 0.20 m CdCl_2 0.20 m LiCl 0.50 m C_3H_6O_3 0.20 m K_3PO_4 Which solution has the LOWEST freezing point? Which solution has the HIGHEST freezing point? The delta H_solution of RbF is 2 kJ/mol.. The lattice energy of RbF is -821 kJ/mol.. What is the sum of the delta H_hydration of Rb^+ (aq) and F^+ (aq) 823 kJ/mol.. -823 kJ/mol.. -819 kJ/mol.. -823 kJ/mol..Explanation / Answer
1) C3H8 will have high boiling point due to high molecular weight
2) H2O will have high boiling point due to hydrgoen bond
3) CF4 will have high boiling point due to more number of electronegative element
4)Cis alkene (A) will have high boiling point due to high london forces
5) Ion dipole forces
6) All are due to hydrophobic forces (water repellant forces)
7) The depression in freezing point is a colligative property and will depend upon the number of ions (molecules) prodcued by the non volatile solute
a) 0.2m CdCl2 : three ions with each 0.2m concentration = 0.6 molal ions
b) 0.2m Licl : two ions with each 0.2m concentration = 0.4 molal ions
c) 0.5m C3H6O3 (dont know wheter it is electrolytic or not so cannot comment), wo we will consider it is non electrolyte
d) 0.2m K3PO4 : total four ions, total concentration 0.8 m
So it will have highest number of ions so maximum depression in freezing poin
A) lowest freezing point : K3PO$
B) Highest : 0.2 M LiCl
C) We know that
Enthalpy of solution = Hydration energy - lattic energy
2 KJ = Hydration energyy - (-821)
Hydration energy = 823 KJ / mole