$A$ binary liquid solution is prepared by mixing $n$-heptane and ethanol. Which one of the following statements is correct regarding the behaviour of the solution?
- AThe solution is non-ideal,showing $-ve$ deviation from Raoult's Law.
- BThe solution is non-ideal,showing $+ve$ deviation from Raoult's Law.
- C$n$-heptane shows $+ve$ deviation while ethanol shows $-ve$ deviation from Raoult's Law.
- DThe solution formed is an ideal solution.
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Similar Questions
The vapour pressures of chloroform $(CHCl_3)$ and dichloromethane $(CH_2Cl_2)$ at $298 \ K$ are $200 \ mmHg$ and $415 \ mmHg$,respectively. An ideal solution is prepared by mixing $59.75 \ g$ of $CHCl_3$ and $21.25 \ g$ of $CH_2Cl_2$. The mole fractions of chloroform and dichloromethane in the vapour phase,respectively,are:
Two liquids $A$ and $B$ have vapour pressure in the ratio $P_A^o : P_B^o = 1 : 3$ at a certain temperature. Assume $A$ and $B$ form an ideal solution and the ratio of mole fractions of $A$ to $B$ in the vapour phase is $4 : 3$. Then the mole fraction of $B$ in the solution at the same temperature is
Difficult
View SolutionFormation of a solution from two components can be considered as
$(i)$ Pure solvent $\to$ separated solvent molecules $\Delta H_1$
$(ii)$ Pure solute $\to$ separated solute molecules $\Delta H_2$
$(iii)$ Separated solvent and solute molecules $\to$ solution $\Delta H_3$
Solution so formed will be ideal if
$(i)$ Pure solvent $\to$ separated solvent molecules $\Delta H_1$
$(ii)$ Pure solute $\to$ separated solute molecules $\Delta H_2$
$(iii)$ Separated solvent and solute molecules $\to$ solution $\Delta H_3$
Solution so formed will be ideal if
MediumAIPMT 2003
View SolutionWhich of the following mixtures forms an ideal solution?
$A$ solution of two liquids boils at a temperature higher than the boiling point of either of them. Hence,the binary solution shows:
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