For which of the following mixtures is Delta_ | vedclass

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Question

(C) Mixtures that exhibit $\Delta_{mix} H > 0$ show a positive deviation from Raoult's law. In such mixtures, the solute-solvent interactions are weak

Vedclass · Accepted Answer

$C_2H_5OH + CH_3COCH_3$

Vedclass · Answer

(C) Mixtures that exhibit $\Delta_{mix} H > 0$ show a positive deviation from Raoult's law. In such mixtures, the solute-solvent interactions are weaker than the solute-solute and solvent-solvent interactions present in the pure components. This results in the absorption of heat upon mixing, making the process endothermic $(\Delta_{mix} H > 0)$. Option $(A)$ $(CHCl_3 + CH_3COCH_3)$ shows negative deviation due to strong hydrogen bonding. Option $(B)$ $(C_6H_5NH_2 + C_6H_5OH)$ shows negative deviation due to acid-base interaction. Option $(C)$ $(C_2H_5OH + CH_3COCH_3)$ shows positive deviation because the strong hydrogen bonds in pure ethanol are disrupted when acetone is added, and the new interactions are weaker. Option $(D)$ $(C_6H_6 + C_6H_5CH_3)$ forms an ideal solution with $\Delta_{mix} H \approx 0$. Therefore, the correct option is $(C)$.

For which of the following mixtures is $\Delta_{mix} H > 0$?

Similar Questions

Which of the following is/are "not correct" for $CH_3OH + CH_3COOH$ mixture solution?
$(a)$ $\Delta H_{\text{mix}} < 0$
$(b)$ Does not obey Raoult's law
$(c)$ $\Delta H_{\text{mix}} > 0$
$(d)$ An example of ideal solution

For an ideal solution of two components $A$ and $B$,which of the following is true?

Which condition is not satisfied by an ideal solution?

$A$ solution of two miscible liquids showing negative deviation from Raoult's law will have :

Which of the following is a non-ideal solution?

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