Chemistry : Equilibrium

In the reaction $3\mathrm{A} + 2\mathrm{B} \to 2\mathrm{C}$, the equilibrium constant K_c is given by

• $\frac{\left[3\mathrm{A}\right] \mathrm{x}\left[2\mathrm{B}\right]}{\left[\mathrm{C}\right]}$

• $\frac{[\mathrm{A}{]}^3\times [\mathrm{B}]}{\left[\mathrm{C}\right]}$

• $\frac{[\mathrm{C}{]}^2}{[\mathrm{A}{]}^3\times [\mathrm{B}{]}^2}$

• $\frac{\left[\mathrm{C}\right]}{\left[3\mathrm{A}\right]\left[2\mathrm{B}\right]}$

The solubility of Sb₂S₃ in water is 1.0 × 10^-5 mol/L at 298K. What will be its solubility product?

• 108 × 10^-25

• 1.0 × 10^-25

• 144 × 10^-25

• 126 × 10^-24

What will be the pH value of 0.05 M Ba(OH)₂ solution?

• 12

• 13

• 1

• 12.96

N₂ and H₂ in 1 : 3 molar ratio are heated in a closed container having a catalyst. When the following equilibrium ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is attained, the total pressure is 10 atm and mole fraction of NH₃ is 0.60. The equilibrium constant K_P for dissociation of NH₃ is

• 1.333 atm^-2

• 0.75 atm^-2

• 0.75 atm²

• 1.333 atm²

According to Le-Chatelier principle, adding heat a solid and liquid in equilibrium will cause the

• amount of solid to decrease

• amount of liquid to decrease

• temperature to rise

• temperature to fall

Solubility of AgCl at 20$°$C is 1.435 x 10^-3 g/L. The solubility product of AgCl is

• 1 x 10^-5

• 1 x 10^-10

• 1.435 x 10^-5

• 108 x10^-3

At 30$°$C the solubility of Ag₂CO₃ (K_sp=8 x 10^-12) would be greatest in one litre of 

• 0.05 M Na₂CO₃

• 0.05 M AgNO₃

• pure water

• 0.05 N NH₃

Which of the following can behave as an acid as well as base ?

• HCl

• H₂SO₄

• H₂O

• NH₃

Ammonium ion is

• a conjugate acid

• a conjugate base

• neither acid nor a base

• both an acid and a base

Which of the following oxide does not form acidic aqueous solution?

• N₂O₃

• NO₂

• N₂O₅

• NO