The equilibrium vapour pressure of water, ethyl alcohol and acetone at 293 K are 2.34 , 5.85 and 12.36 kPa respectively. Which of these will have the lowest and highest boiling points? At 293 K Which of these will Evaporate least in a sealed container before equilibrium is established ?

The vapour pressures of benzene and toluene at 293 K are 75 mm and 22 mm Hg respectively. 23.4g of benzene and 64.4 g of toluene are mixed. If the two form and ideal solution, calculate the mole fraction of benzene in the vapour phase assuming that the vapours are in equilibrium with the liquid mixture at this temperature.

The vapour pressure of two pure liquids A and B are 200 and 400 tor respectively at 300K. A liquid solution (ideal) of A and B for which the mole fraction of A is 0.40 is contained in a cylinder. The composition of components A and B in vapour phase after equilibrium is reached between vapour & liquid phase, respectively is

Vapour pressure of CH_(3)Cl and CH_(2)Cl_(2) are 540 mm Hg and 402 mm Hg respectively. 101 g of CH_(3)Cl and 85 g of CH_(2)Cl_(2) are mixed together. Determine (i) The pressure at which the solution starts boiling. (ii) Molar ratio of solute v/s solvent in vapour phase in equilibrium with solution.

Vapour pressure of CH_(3)Cl and CH_(2)Cl_(2) are 540 mm Hg and 402 mm Hg respectively. 101 g of CH_(3)Cl and 85 g of CH_(2)Cl_(2) are mixed together. Determine (i) The pressure at which the solution starts boiling. (ii) Molar ratio of solute v/s solvent in vapour phase in equilibrium with solution.

Use the information and data given below to answer the question (a) to (c), Stronger intermolecular forces result in higher boiling point. Strength of London forces increases with the number of electrons in the molecule. Boiling point of HF, HCl, HBr and HI are 293 K, 189 K, 206 K and 238 K respectively. (a) which type of intermolecular forces are present in the molecules HF, HCl, HBr and HI ? (b) Looking at the trend of boiling points of HCl, HBr and HI , explain out of dipole-dipole interaction and London interaction, which one is predominant here. (c) Why is boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest ?

A system of greater disorder of molecules is more probable. The disorder of molecules is reflected by the entropy of the system. A liquid vapourizes to form a more disordered gas. When a solute is present, there is additional contribution to the entropy of the liquid due to increased randomness. As the entropy of solution is higher than that of pure liquid, there is weaker tendency to form the gas. Thus, a solute (non-volatile) lowers the vapour pressure of a liquid, and hence a higher boiling point of the solution. Similarly, the greater randomness of the solution opposes the tendercy to freeze. In consequence, a lower temperature must be reached for achieving the equilibrium between the solid (frozen solvent) and the solution. The elevation in boiling point (DeltaT_(b)) and depression in freezing point (DeltaT_(f)) of a solution are the colligative properties which depend only on the concentration of particles of the solute and not their identity. For dilute solutions, (DeltaT_(b)) and (DeltaT_(f)) are proportional to the molarity of the solute in the solution. To aqueous solution of Nal , increasing amounts of solid Hgl_(2) is added. The vapour pressure of the solution

The ester , ethyl acetate is formed by the reaction of ethanol and acetic acid and the equilibrium is represented as : CH_(3) COOH(l) +C_(2)H_(5)OH(l)hArr CH_(3)COOC_(2)H_(5)(l) +H_(2)O(l) (i) Write the concentration ratio (concentration quotient) Q for this reaction. Note that water is not in excess and is not a solvent in this reaction. (ii) At 293 K, if one starts with 1.000 mol of acetic acid 0.180 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture . Calculate the equilibrium constant. (iii) Starting with 0.50 mol of ethanol and 1.000 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after some time. Has equilibrium been reached?

Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as : CH_3COOH(l) +C_2H_5OH(l) hArr CH_3COOC_2H_5(l) +H_2O(l) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime . Has equilibrium been reached?

The system shown in the figure is in equilibrium, where A and B are isomeric liquids and form an ideal solution at TK . Standard vapour pressures of A and B are P_(A)^(0) and P_(B)^(0) , respectively, at TK . We collect the vapour of A and B in two containers of volume V , first container is maintained at 2 T K and second container is maintained at 3T//2 . At the temperature greater than T K , both A and B exist in only gaseous form. We assume than collected gases behave ideally at 2 T K and there may take place an isomerisation reaction in which A gets converted into B by first-order kinetics reaction given as: Aoverset(k)rarrB , where k is a rate constant. In container ( II ) at the given temperature 3T//2 , A and B are ideal in nature and non reacting in nature. A small pin hole is made into container. We can determine the initial rate of effusion of both gases in vacuum by the expression r=K.(P)/(sqrt(M_(0))) where P= pressure differences between system and surrounding K= positive constant M_(0)= molecular weight of the gas If vapours are collected in a container of volume 8.21 L maintained at 3 T//2K , where T=50 K , then the ratio of initial rate of effusion of gases A and B is given as

The system shown in the figure is in equilibrium, where A and B are isomeric liquids and form an ideal solution at TK . Standard vapour pressures of A and B are P_(A)^(0) and P_(B)^(0) , respectively, at TK . We collect the vapour of A and B in two containers of volume V , first container is maintained at 2 T K and second container is maintained at 3T//2 . At the temperature greater than T K , both A and B exist in only gaseous form. We assume than collected gases behave ideally at 2 T K and there may take place an isomerisation reaction in which A gets converted into B by first-order kinetics reaction given as: Aoverset(k)rarrB , where k is a rate constant. In container ( II ) at the given temperature 3T//2 , A and B are ideal in nature and non reacting in nature. A small pin hole is made into container. We can determine the initial rate of effusion of both gases in vacuum by the expression r=K.(P)/(sqrt(M_(0))) where P= pressure differences between system and surrounding K= positive constant M_(0)= molecular weight of the gas Vapours of A and B are passed into a container of volume 8.21 L , maintained at 2T K , where T=50 K and after 5 min , moles of B=8//3 . The pressure developed into the cotainer after two half lives is