61.

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

• MnO₂

• H₂S

• KMnO₄

• Cr₂O₃

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

• 6y⁴

• 36y⁴

• 64y⁵

• 108y⁵

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

What is the conjugate base of OH ?

• O₂

• H₂O

• O^-

• O^2-

The conjugate base of NH${}_2^{-}$ is

• NH₃

• NH^2-

• NH${}_4^{+}$

• N${}_3^{-}$

In an amino acid, the carboxyl group ionises at p${\mathrm{k}}_{{\mathrm{a}}_1}$ = 2.34 and ammonium, ion at p${\mathrm{k}}_{{\mathrm{a}}_2}$ = 9.6. The isoelectric point of the amino acid is at pH

• 5.97

• 11.94

• 2.34

• 9.60

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

Consider the water gas equilibrium reaction,

C (s) + H₂O (g) $\rightleftharpoons$ 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 H₂ would be formed

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

      ${\mathrm{CH}}_3{\mathrm{COOC}}_2{\mathrm{H}}_5 + {\mathrm{H}}_2\mathrm{O} \rightleftharpoons {\mathrm{CH}}_3\mathrm{COOH} + {\mathrm{C}}_2{\mathrm{H}}_5\mathrm{OH}$

• 33.7

• 7.33

• 5.33

• 33.3

The reaction

           2A(g) + B(g) $\rightleftharpoons$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)² (0.25)]