The vapour pressure of pure liquid solvent A is atm. When a non-volatile substance B is added to the solvent, its vapour pressure drops to 0.60 atm. What is the mole fraction of component B in the solution?
The freezing point of a solution composed of 10.0 g of KCl in 100 g of water is \[4.5{}^\circ C\]. Calculate the van't Hoff factor, i for this solution.
A mixture of A and B, which are two miscible liquids, is distilled under equilibrium conditions at atmospheric pressure. The mole fraction of A in solution is 0.3 and in vapour phase is 0.6. If the solution behaves ideally the ratio of \[P\,_{A}^{o}\] to \[P\,_{B}^{o}\] is
The partial pressure of \[C{{O}_{2}}\] in air saturated with water vapours at \[25{}^\circ C\] and 1.00 atm is \[3.04\times {{10}^{-4}}\] atm. Henry's constant for \[C{{O}_{2}}\] in water is \[2.3\times {{10}^{-2}}\,\text{mol}\,{{\text{L}}^{-1}}\text{at}{{\text{m}}^{-1}}\] and for carbonic acid \[p{{K}_{a}}\] is 6.37. The pH of normal (\[C{{O}_{2}}\] mixed) rain water will be
Normal boiling point of water is 373 K (at 760 mm). Vapor pressure of water at 298 K is 23 mm. If the enthalpy of evaporation is 40.656 kJ/mol, the boiling point of water at 23 mm pressure will be:
A compound has the empirical formula\[{{C}_{10}}{{H}_{8}}Fe\]. A solution of 0.26 g of the compound in 11.2 g of benzene \[({{C}_{6}}{{H}_{6}})\] boils at \[\text{8}0.\text{26}{}^\circ \text{C}\]. The boiling point of benzene is \[\text{8}0.\text{1}0{}^\circ \text{C}\] and \[{{K}_{b}}\] is \[\text{2}.\text{53}{}^\circ \text{C}/\text{molal}.\]
Two components A and B form an ideal solution. The mole fraction of A and B in ideal solutions are \[{{X}_{A}}\] and \[{{X}_{B}},\] while that of in vapour phase, these components have their mole fractions as \[{{Y}_{A}}\] and \[{{Y}_{B}}\] then, the slope and intercept of plot of \[\frac{1}{{{Y}_{A}}}\] us \[\frac{1}{{{X}_{A}}}\] will be
When 2g of non-volatile hydrocarbon containing 94.4 percent carbon is dissolved in 100g benzene, the vapour pressure of Benzene is lowered from 74.66 torr to 74.01 torr. Determine the molecular formula of the hydrocarbon.
A solution of 0.2 mole \[Kl\]\[(\alpha =100\,%)\] in 1000 g water freezes at \[{{T}_{1}}{{\,}^{0}}C\]. Now to this solution 0.1 mole \[Hg{{I}_{2}}\] is added and the resulting solution freezes at \[{{T}_{2}}{{\,}^{0}}C\]. Which of the following is correct:
At \[20{}^\circ C\] and 1.00 atm partial pressure of hydrogen, 18 mL of hydrogen, measured at STP, dissolves in 1L of water. If water at \[20{}^\circ C\]is exposed to a gaseous mixture having a total pressure of 1400 Torr (excluding the vapour pressure of water) and containing 68.5% \[{{H}_{2}}\] by volume, find the volume of \[{{H}_{2}},\] measured at STP, which will dissolve in 1L of water.
The vapour pressure of two pure liquids A and B which form an ideal solution are 1000 and 1600 torr respectively at 400 K. A liquid solution of A and B for which the mole fraction of A is 0.60 is contained in a cylinder by a piston on which the pressure can be varied. The solution use slowly vapourised at 400 K by decreasing the applied pressure. What is the composition of last droplet of liquid remaining in equilibrium with vapour?
Vapour pressure of \[CC{{l}_{4}}\] at \[{{25}^{o}}C\] is 143 mm of Hg. 0.5 gm of a non-volatile solute (mol. wt. = 65) is dissolved in 100 ml \[CC{{l}_{4}}.\] Find the vapour pressure of the solution (Density of \[CC{{l}_{4}}=1.54\,g.c{{m}^{3}}\])
A 0.001 molal solution of \[\left[ Pt{{\left( N{{H}_{3}} \right)}_{4}}C{{l}_{4}} \right]\] in water had a freezing point depression of\[0.0054{}^\circ C\]. If \[{{K}_{f}}\] for water is 1.80, the correct formulation for the above molecule is:
Boiling point of chloroform was raised by 0.323 K, when 0.5143 g of anthracene was dissolved in 35 g of chloroform. Molecular mass of anthracene is: (\[{{K}_{b}}\] for \[CHC{{l}_{3}}\]= 3.9 kg/mol )
The ratio of \[\Delta {{T}_{f}}\] for \[{{K}_{4}}[Fe{{(CN)}_{6}}]\] solution (assuming complete ionization) to \[\Delta {{T}_{f}}\] for solution of sugar of equal concentration is
Suppose 5 gm of \[C{{H}_{3}}COOH\] is dissolved in one litre of ethanol. Assume that no reaction between them takes place. Calculate molality of resulting solution if density of ethanol is 0.789 gm/ml.
The vapour pressure curves of the same solute in the same solvent are shown. The curves are parallel to each other and do not intersect. The concentrations of solutions are in order of:
An aqueous solution containing liquid A \[(M.\,\,Wt.=128)\] 64% by weight has a vapour pressure of 145 mm. Find the vapour pressure of pure A. If that of water is 155 mm at the same temperature.
The total vapor pressure of a mixture of 1 mol of volatile component A (\[P_{A}^{O}\]= 100 mm Hg) and 3 mol of volatile component B (\[P_{B}^{O}\]=80 mm Hg) is 90 mm Hg. For such case:
A)
there is a positive deviation from Raoult's law
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B)
boiling point has been lowered
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C)
force of attraction between A and B is smaller than that between A and A or between B and B
Concentrated \[HN{{O}_{3}}\] is 63% \[HN{{O}_{3}}\] by mass and has a density of 1.4 g/mL. How many millilitres of this solution are required to prepare 250 mL of a 1.20 M \[HN{{O}_{3}}\] solution?
