For a phase changeH2O(l)   ⇌0°C, 1&

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641.

For a phase change

H2O(l)   0°C, 1 bar  H2O(s)

  • G = 0

  • H = 0

  • S =0

  • U = 0


A.

G = 0

G°=-RTlnK  [G°= standard free energy change, K = equilibrium constant]

If a substance is in equilibrium between two phases at constant temperature and pressure, its chemical potential must have the same value in both the phases. Therefore G°=0.


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642.

F2 formed by reacting K2MnF6 with

  • SbF5

  • MnF3

  • KSbF6

  • MnF4


643.

Which among the following is the strongest acid ?

  • HF

  • HCl

  • HBr

  • HI


644.

When 10 mL of 0.1 M acetic acid (pK= 5.0) is titrated against 10 ml of 0.1 M ammonia solution (pK= 5.0), the equivalence point occurs at pH

  • 5.0

  • 6.0

  • 7.0

  • 9.0


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645.

For reaction, 2NOCl (g) 2NO (g) + Cl2 (g), Kc at 427°C is 3 × 10-6 L mol-1. The value of Kp is nearly

  • 7.50 × 10-5

  • 2.50 × 10-5

  • 2.50 × 10-4

  • 1.75 × 10-4


646.

For the chemical equilibrium,

CaCO3(s) CaO(s) + CO2(g)

Hr° can be determined from which one of the following plots?


647.

pH of a solution of 10 mL 1N sodium acetate and 50 mL 2N acetic acid (Ka = 1.8 x 10-5), is approximately :

  • 4

  • 5

  • 6

  • 7


648.

The pH is less than 7, of the solution of :

  • FeCl3

  • NaCN

  • NaOH

  • NaCl


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649.

Dimethyl glyoxime gives a red precipitate with Ni2+, which is used for its detection. To get this precipitate readily the best pH range is

  • < 1

  • 2-3

  • 3- 4

  • 9- 11


650.

The values of Ksp for CuS, Ag2S and HgS are 10-31, 1042, 10-54 respectively. The correct order of their solubility in water is :

  • AgS > HgS > CuS

  • HgS > Cus > Ag2S

  • HgS > Ag2S > Cus

  • Ag2S > CuS > HgS


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