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Class XI Chemistry Equilibrium 2

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Question 1

The equilibrium constant expression for the equilibrium
2NH₃(g) + 2O₂(g) N₂O(g) + 3H₂O(g) is

Question 2

The value of K_P for the reaction.
2H₂O(g) + 2Cl₂(g) 4HCl (g) + O₂(g)
is 0.03 atm at 427 ºC, when the partial pressure are expressed in atmosphere, then the value of K_C for the same reaction is -

Question 3

0.1 mole of N₂O_4(g) was sealed in a tube under one atmospheric conditions at 25^oC. Calculate the number of moles of NO_2(g) present, if the Equlibrium

is reached after some time

Question 4

For the reaction equilibrium, N₂O₄(g) ---> 2NO₂ (g),the concentrations of N₂O₄ and NO₂ gas, at equilibrium are 4.8 10^–2 mol L^–1 and 1.2 10^–2 mol L^–1respectively. The value of K_c for the reaction is

Question 5

The equilibrium constant at 298 K for a reaction

is 100. If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L^-1) will be :

Question 6

The solubility in water of a sparingly soluble salt AB₂ is

mol L^–1. Its solubility product number will be

Question 7

For the reaction
2NO_{2 (g)}

2NO_(g) + O_{2 (g)}
(K_c = 1.8 × 10^-6 at 184 °C)
(R = 0.0831 kJ / (mol K)
When K_p and K_c are compared at 184 °C, it's found that

Question 8

Solid Ba(NO₃)₂ is gradually dissolved in a 1.0 × 10^–4M Na₂CO₃ solution. At what concentration of Ba²⁺ will a precipitate being to form? (K_sp for Ba CO₃ = 5.1 × 10^–9):

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