Which of the following are correct for an ide | vedclass

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(C) An ideal solution is a solution that obeys Raoult's law over the entire range of concentration.Such solutions are formed by mixing two components

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$a, b, c$ only

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(C) An ideal solution is a solution that obeys Raoult's law over the entire range of concentration.Such solutions are formed by mixing two components that are similar in molecular size, structure, and have almost identical intermolecular forces.The characteristics of ideal solutions are:$(1)$ It must obey Raoult's law.$(2)$ The enthalpy of mixing should be zero, i.e.,$\Delta H_{	ext{mix}} = 0$.$(3)$ The volume of mixing should be zero, i.e.,$\Delta V_{	ext{mix}} = 0$, which implies $V_{	ext{solvent}} + V_{	ext{solute}} = V_{	ext{solution}}$.Examples of ideal solutions include $n$-hexane + $n$-heptane and benzene + toluene.The mixture of carbon dioxide and water is not an ideal solution because they react with each other to form $H_2CO_3$, which involves chemical changes and significant enthalpy changes.Therefore, statements $(a)$, $(b)$, and $(c)$ are correct.

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.

Similar Questions

The formation of a binary solution is considered as follows:
$(1)$ Pure solvent enthalpy $\Delta H_1$ (separated)
$(2)$ Pure solute enthalpy $\Delta H_2$ (separated)
$(3)$ Pure solvent + Pure solute $\to$ Solution $\to$ Enthalpy $\Delta H_3$
If $......$ then the resulting solution is ideal.

At $27^o C$,the vapor pressure of pure liquid $A$ is $70 \ torr$. It forms an ideal solution with $B$. The mole fraction of $B$ is $0.2$ and the vapor pressure of the solution at $27^o C$ is $84 \ torr$. What is the vapor pressure of pure liquid $B$ at $27^o C$ (in $torr$)?

$A$ solution of two liquids boils at a temperature higher than the boiling point of either of them. Hence,the binary solution shows:

In a mixture of components $A$ and $B$,the components show negative deviation when:

At $300 \ K$,the vapour pressures of $A$ and $B$ liquids are $500 \ mm \ Hg$ and $400 \ mm \ Hg$ respectively. Equal moles of $A$ and $B$ are mixed to form an ideal solution. The mole fraction of $A$ and $B$ in the vapor state is respectively:

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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.