Equilibrium Tes...

Direction (Q. Nos. 1-13) This section contains 13 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.

Q. Given the reactions, If one mole each of A and B are take in 5 L flask at 300 K, 0.7 mole of C are formed. Molar concentration of each species at equilibrium, when one mole of each are taken initially is

On taking 60.0 g CH₃COOH and 46.0 g CH₃CH₂OH in a 5 L flask in the presence of H₃0⁺ (catalyst), at 298 K 44.0 g of CH₃COOC₂H₅ is formed at equilibrium.

If amount of CH₃COOH is doubled without affecting amount of CH₃CH₂OH, then CH₃COOC₂H₅ formed is 

For the reversible reaction, 

In a reaction vessel, [NO]= [O₂]= 0.01 mol L^-1 and [NO₂]= 0.1 mol L^-1 then above reaction is 

The equilibrium constant for the following reaction, is 1.6 x 10⁵ at 1024 K.

H₂(g) + Br₂(g) ⇌2HBr(g)
HBr (g)at 10.0 bar is introduced into a sealed container at 1024 K. Thus, partial pressure of H₂(g)and Br₂(g), together is

At 273 K and 1 atm, 1 L of N₂O₄ (g) decomposes to NO₂(g)a s given,

N₂O₄(g) ⇌2NO₂(g)

At equilibrium, original volume is 25% less than the existing volume. Percentage decomposition of N₂O₄ (g) is thus, 

H₂S (g) initially at a pressure of 10.0 atm and a temperature of 800 K, dissociates as

2H₂S(g) ⇌ 2H₂(g) + S₂(g)

At equilibrium, the partial pressure of S₂ vapour is 0.020 atm . Thus, K_p is 

A sample of N₂O₄(g)with a pressure of 1.00 atm is placed in a flask. When equilibrium is reached, 20% of N₂O₄(g)has been converted to NO₂(g)

If the original pressure is made 10% of the earlier pressure, then per cent dissociation will be

Following equilibrium is set up at 1000 K and 1 bar in a 5 L flask,

At equilibrium, NO₂ is 50% o f the total volume. Thus, equilibrium constant K_c is 

Following equilibrium is set up at 298 K in a 1 L flask.

If one starts with 2 moles of A and 1 mole of B, it is found that moles of B and D are equal.Thus K_c is 

At 700 K and 350 bar, a 1 : 3 mixture of N₂(g) and H₂(g) reacts to form an equilibrium mixture containing X (NH₃)= 0.50. Assuming ideal behaviour K_p for the equilibrium reaction, 

Equilibrium constant for the reaction,

is 1.8 x 109. Hence, equilibrium constant for

A gaseous phase reaction taking place in 1L flask at 400 K is given, 

Starting with 1 mole N₂ and 3 moles H₂, equilibrium mixture required 250 mL of 1M H₂SO₄ . Thus, K_c is 

For the following equilibrium starting with 2 moles SO₂ and 1 mole O₂ in 1 L flask,

Equilibrium mixture required 0.4 mole in acidic medium. Hence, K_c is 

Direction (Q. Nos. 14 and 15) This sectionis based on statement I and Statement II. Select the correct answer from the code given below.

Q. Statement I 

If K_c = 4 for the following equilibrium,

Then mixture of 1 mole N₂, 3 moles H₂ and 2 moles NH₃ in 1L flask is in equilibrium.

Statement II

Reaction quotient of the given quantities is less than the equilibrium constant.

Statement I

1 mole A(g) and 1 mole B(g)give 0.5 mole of C(g)and 0.5 mole D(g) at equilibrium.

On taking 2 moles each of A(g)and B(g), percentage dissociation A(g)and B(g) is also doubled.

Statement II

Equilibrium constant, K_c = 1