Consider the following liquid-vapor equilibrium Liquid ↔ Vapour Which of the following relation is correct?

$\frac{dlnp}{dT}=\frac{\Delta H_v}{RT^2}$

$\frac{dlnp}{dT}=\frac{-\Delta H_v}{RT}$

$\frac{dlnp}{dT^2}=\frac{-\Delta H_v}{T^2}$

$\frac{dlnG}{dT^2}=\frac{-\Delta H_v}{RT^2}$

For an ideal solution, the non zero value will be for-

$\Delta P=P_{\text{observed}}-P_{\text{Raoult}}$

The boiling point of 0.2 mol kg -1 solution of X in water is greater than equimolal solution of Y in water. The correct statements in this case is-

X is undergoing dissociation in water.

Molecular mass of X is greater than the molecular mass of Y.

Molecular mass of X is less he molecular mass of y.

Y is undergoing dissociation in water while X undergoes no change.

Chemistry - Solutions - Quiz-6

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Of the following 0.10m aqueous solutions, the one will exhibit the largest freezing point depression is-

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KCl
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$C_{6} H_{12} O_{6}$
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${Al}_{2} ({SO}_{4})_{3}$
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$K_{2} {SO}_{4}$

The freezing point depression constant for water is -1.86

$°$ C m^-1. If 5.00 g Na₂SO₄is dissolved in 45.0 g H₂O, the freezing point is changed by -3.82

$°$ C. The van’t Hoff factor for Na₂SO₄ is-

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2.63
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3.11
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0.381
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2.05

A solution containing 10g per dm³ of urea (molecular mass = 60g mol^-1) is isotonic with a 5% solution of a non-volatile solute. The molecular mass of this non-volatile solute is -

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25g mol^-1.
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300g mol^-1.
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350g mol^-1.
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200g mol^-1.

During osmosis, the flow of water through a semi-permeable membrane is -

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From a solution having higher concentration only
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From both sides of the semi-permeable membrane with equal flow rates
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From both sides of the semi-permeable membrane with unequal flow rates
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From a solution having lower concentration only

The mixture that forms maximum boiling azeotrope is-

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Heptane+Octane
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Water+Nitric acid
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Ethanol +Water
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Acetone+Carbon disulfide

$C_{6} H_{6}$ freezes at 5.5 $°$ C. At what temperature will a solution of 10.44 g of $C_{4} H_{10}$ in 200 g of $C_{6} H_{6}$ freeze ? K_f ( $C_{6} H_{6}$ ) = 5.12 $°$ C/m

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4.60 $°$ C
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0.89 $°$ C
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5.50 $°$ C
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None of the above

The Henry's law constant for the solubility of N₂ gas in water at 298 K is 1.0 × 10⁵ atm. The mole fraction of N₂ in air is 0.8. The number of moles of N₂ from air dissolved in 10 moles of water at 298 K and 5 atm pressure is-

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4.0 × 10^–4
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4.0 × 10^–5
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5.0 × 10^–4
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4.0 × 10^–6

If the relative decrease in vapour pressure is 0.4 for a solution containing 1 mol NaCl in 3 mol of $H_{2} O$ , then percentage ionisation of NaCl will be -

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60%
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80%
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40%
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100%

Boiling of dil. HCl acid does not increase its concentration beyond 22.2 per cent because hydrochloric acid:

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is very volatile
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is extremely soluble in water
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forms a constant boiling mixture
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forms a saturated solution at this concentration

A 500 g toothpaste sample has 0.4 g fluoride concentration. The fluoride concentration in terms of ppm will be -

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200
0%

400
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500
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800

The correct statement regarding a solution of two component A and B exhibiting positive deviation from idea behavior is -

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Intermolecular attractive force between A-A and B-B are stronger than those between A-B
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$∆_{m i x} H = 0 a t c o n s \tan t T a n d P$
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$∆_{m i x} V = 0 a t c o n s \tan t T a n d P$
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Intermolecular attractive forces between A-A and B-B are equal to those between A-B

The correct sequence of order of increasing solubility in the n-octane is-

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Cyclohexane < CH₃CN < CH₃OH < KCl
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KCl < CH₃OH < CH₃CN < Cyclohexane
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KCl < CH₃OH > CH₃CN < Cyclohexane
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None of the above

17.4% (w/v) $K_{2} {SO}_{4}$ solution at 27 $°$ C is isotonic to 5.85% (w/V) NaCl solution at 27 $°$ C. lf

NaCl is 100% ionised, the % ionisation of $K_{2} {SO}_{4}$ in aqueous solution is-

[At wt. of K= 39,Na =23] :-

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25%
0%

75%
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50%
0%

None of the above

The vapor pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in the vapor phase in contact with an equimolar solution of benzene and toluene is:

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0.50
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0.6
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0.27
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0.73

The mixture shows positive deviation from Raoult's law is-

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Benzene + Toluene
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Acetone + Chloroform
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Chloroethane + Bromoethane
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Ethanol + Acetone

The freezing point of depression constant $(K_{f})$ of benzene is 5.12 K kg ${mol}^{- 1}$ . The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is- (rounded off upto two decimal places) :

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0.80 K
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0.40 K
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0.60 K
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0.20 K

For a solution, the plot of osmotic pressure ( $π$ ) versus the concentration (c in mol L^-1) gives a straight line with slope 310R where 'R' is the gas constant. The temperature at which osmotic pressure measured is -

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310 × 0.082 K
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310 $^{o}$ C
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37 $^{o}$ C
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$\frac{310}{0.082} K$

For the dissociation of PCl₅ into PCl₃ and Cl₂ in gaseous phase reaction, if d is the observed vapour density and D the theoretical vapour density with 'a' as degree of dissociation. Variation of D/d with 'a' is given by which graph