$A$ 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
Which of the following pairs does not form an ideal solution?
Easy
View SolutionOn mixing,heptane and octane form an ideal solution. At $373 \ K$,the vapour pressures of the two liquid components (heptane and octane) are $105 \ kPa$ and $45 \ kPa$ respectively. Vapour pressure of the solution obtained by mixing $25.0 \ g$ of heptane and $35 \ g$ of octane will be $........ \ kPa$.
(molar mass of heptane $= 100 \ g \ mol^{-1}$ and of octane $= 114 \ g \ mol^{-1}$)
(molar mass of heptane $= 100 \ g \ mol^{-1}$ and of octane $= 114 \ g \ mol^{-1}$)
DifficultAIEEE 2010
View SolutionWhich 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.
Which of the following pairs of liquids shows a negative deviation from Raoult's law?
Easy
View Solution$1 \, \text{mole}$ of liquid $A$ and $2 \, \text{mole}$ of liquid $B$ form a solution with a vapor pressure of $38 \, \text{torr}$. If the vapor pressures of pure $A$ and pure $B$ are $45 \, \text{torr}$ and $36 \, \text{torr}$ respectively,the solution will be:
Easy
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