In a mixture of $A$ and $B$ components,the solution shows positive deviation from Raoult's law when:
- A$A-B$ interaction is stronger than $A-A$ and $B-B$ interaction
- B$A-B$ interaction is weaker than $A-A$ and $B-B$ interaction
- C$\Delta V_{mix} < 0$,$\Delta S_{mix} > 0$
- D$\Delta V_{mix} = 0$,$\Delta S_{mix} > 0$
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At a particular temperature,the vapour pressures of two liquids $A$ and $B$ are respectively $120 \, mm$ and $180 \, mm$ of mercury. If $2 \, moles$ of $A$ and $3 \, moles$ of $B$ are mixed to form an ideal solution,the vapour pressure of the solution at the same temperature will be (in $mm$ of mercury):
MediumAIIMS 2013
View SolutionFor the ideal solutions,which of the following condition is suitable?
Which of the following are correct for an ideal solution?
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.
$(a) \Delta V_{\text{mix}} = 0$
$(b) V_{\text{solvent}} + V_{\text{solute}} = V_{\text{solution}}$
$(c) \Delta H_{\text{mix}} = 0$
$(d) H_2O + CO_2 \rightarrow H_2CO_3$ is an example of an ideal solution.
The mixture which shows positive deviation from Raoult's law is
MediumNEET 2020
View SolutionAn ideal solution has two components $A$ and $B$. If $A$ is more volatile than $B$,then the correct relation between mole fraction of $A$ in liquid $(X_A)$ and vapour phase $(Y_A)$ is:
Medium
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