Which of the following is used to prepare Cl2 gas at room te

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61.

Which of the following is used to prepare Cl2 gas at room temperature from concentrated HCl?

  • MnO2

  • H2S

  • KMnO4

  • Cr2O3


C.

KMnO4

KMnO4 is used to prepare Cl2 gas at room temperature from concentrated HCl.


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62.

The solubility of Ca3(PO4)2 in water is y mol/L. Its solubility product is

  • 6y4

  • 36y4

  • 64y5

  • 108y5


63.

A compound on burning in air produces three oxides. Out of these one oxide turns lime water milky, the second one turned anhydrous CuSO4 blue and third forms a solution of pH = 9. The compound is made up of

  • S, N and H

  • S, H and Na

  • S and N

  • S, C and H


64.

What is the conjugate base of OH ?

  • O2

  • H2O

  • O-

  • O2-


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65.

The conjugate base of NH2- is

  • NH3

  • NH2-

  • NH4+

  • N3-


66.

In an amino acid, the carboxyl group ionises at pka1 = 2.34 and ammonium, ion at pka2 = 9.6. The isoelectric point of the amino acid is at pH

  • 5.97

  • 11.94

  • 2.34

  • 9.60


67.

The solubility product of Ag2CrO4 is 32 x 10-12.What is the concentration of CrO4- ions in that solution?

  • 2x 10-4 M

  • 16x 10-4 M

  • 8x 10-4 M

  • 8x 10-8 M


68.

Consider the water gas equilibrium reaction,

C (s) + H2O (g)  CO (g) + H2 (g)

Which of the following statements is true at equilibrium?

  • If the amount of C(s) is increased, less water would be formed

  • If the amount of C(s) is increased, more CO and H2 would be formed

  • If the pressure on the system is increased by halving the volume, more water would be formed

  • If the pressure on the system is increased by halving the volume, more CO and Hwould be formed


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69.

The rate constant for forward reaction and backward reaction of hydrolysis of ester are 1.1 x10-2 and 1.5 x10-3 per minute respectively. Equilibrium constant for the reaction is

      CH3COOC2H5 + H2O  CH3COOH + C2H5OH

  • 33.7

  • 7.33

  • 5.33

  • 33.3


70.

The reaction

           2A(g) + B(g) 3C(g) + D(g)

is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression

  • [(0.75)3 (0.25)] ÷ [(1.00)2 (1.00)]

  • [(0.75)3 (0.25)] ÷ [(0.50)2 (0.75)]

  • [(0.75)3 (0.25)] ÷ [(0.50)2 (0.25)]

  • [(0.75)3 (0.25)] ÷ [(0.75)(0.25)]


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