Answer:
The correct answer will be " RbF > RbCl > RbBr > Rbl".
Explanation:
The size of the given ions will be:
<u>RbCl:</u>
⇒ 689kJ/mol
<u>RbBr:</u>
⇒ 660kJ/mol
<u>Rbl:</u>
⇒ 630kJ/mol
<u>RbF:</u>
⇒ 785kJ/mol
Now according to the size, the arrangement will be:
⇒ (785kJ/mol) > (689kJ/mol) > (660kJ/mol) >(630kJ/mol)
⇒ RbF > RbCl > RbBr > Rbl
The bond among all opposite charging ions seems to be strongest whenever the ions were indeed small.
Answer: Option (c) is the correct answer.
Explanation:
A binary mixture is defined as the mixture which contains two components in the aqueous medium. The two components are solute and solvent.
And, volatility is defined as the ability of a liquid solution or substance to readily change into vapors.
For a binary solution the expression for relative volatility is as follows.
= 
where, 
= relative volatility of more volatile component i
= vapor-liquid equilibrium concentration of component i in the vapor phase
= vapor-liquid equilibrium concentration of component i in the liquid phase
= vapor-liquid equilibrium concentration of component j in the vapor phase
= vapor-liquid equilibrium concentration of component j in the liquid phase
So, when > 1 then separation by distillation is easier in nature.
Thus, we can conclude that in order to separate the components of a binary mixture, the relative volatility should be greater than unity.
The solution is unsaturated.
Supersaturated is when you put so much powder it no longer dissolves.
