Chemical Equilibrium Test

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Chemical Equilibrium Test - 12

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Weekly Quiz Competition

Question 1
1 / -0

If K_p for a reaction, A(g)+2B(g) ⇌ 3C(g) + D(g) is 0.05 atm at 1000K, its K_c in terms of R will be:

A
20000R

B
0.02R

C
5×10⁻⁵ R

D

Solution

For the reaction A(g) + 2B(g) ⇌ 3C(g) + D(g)

Δn = 3 + 1 − (1+2) = 1

K_p = K_c(RT)^Δn

0.05 = K_c × (R×1000)¹
Question 2
1 / -0

The vapour density of N₂O₄ at a certain temperature is 30. What is the percentage dissociation of N₂O₄ at this temperature ?

A
53.3%

B
106.6%

C
26.7%

D
None.

Solution
Question 3
1 / -0

If PCl₅ is 80% dissociated at 523 K, what is the vapour density of the equilibrium mixture at 523 K ?

A
57.92

B
67.92

C
77.93

D
45.45

Solution

The correct option is A 57.92
PCl₅(s) ⇌ PCl₃(g) + Cl₂(g)
n = 2
α = 80% = 80/100 = 0.8
theoretical vapour/Normal vapour density,

D = Normal molar mass/2 = 208.5/2 = 104.25

vapour density of the equilibrium mixture, d=?
we have the relation
Question 4
1 / -0

Ammonium carbamate when heated to 200⁰C gives a mixture of NH₃ and CO₂ with vapour density of 13.

The degree of dissociation of ammonium carbonate is:

A
1

B
0.5

C
0.75

D
0.9

Solution
Question 5
1 / -0

In the reaction, H₂(g)+I₂(g) ⇌ 2HI(g) the concentration of H₂, I₂ and HI at equilibrium are 8.0, 3.0 and 28 moles per litre respectively. What will be the equilibrium constant ?

A
30.61

B
32.66

C
29.40

D
20.90

Solution

H₂(g)+I₂(g)⇌2HI(g)

Applying law of mass action,

Given : [H₂]=8.0 mol L−1, [I₂]=3.0 mol L⁻¹ ,[HI]=28.0 mol L^−I
Question 6
1 / -0

For the reaction, N₂(g) + 3H₂(g) ⇌ 2NH₃(g), the partial pressures of N₂ and H₂ are 0.80 and 0.40 atmosphere respectively at equilibrium. The total pressure of the system is 2.80 atmosphere. What is K_p for the above reaction?

A
32 atm^-2

B
20 atm^-2

C
50 atm^-2

D
80 atm^-2

Solution
Question 7
1 / -0

A two litre flask contains 1.4 gm nitrogen and 1.0 gm hydrogen. The ratio of active mass of nitrogen and hydrogen would be -

A
1 : 3

B
1 : 5

C
1.4 : 1

D
1 : 10

Solution
Question 8
1 / -0

The reaction A(g)+B(g) ⇋ C(g)+D(g) is studied in a one litre vessel at 250^∘C. The initial concentration of A was 3n and that of B was n. When equilibrium was attained, equilibrium concentration of C was found to be equal to the equilibrium concentration of B. What is the concentration of D at equilibrium?

A
n/2

B
(3n−1/2)

C
(n−n/3)

D
n

Solution
Question 9
1 / -0

The value of K_c for the reaction :

A + 3 B ⇌ 2C at 400°C is 0.5. Calculate the value of K_P

A
1.64×10⁻⁴

B
1.64×10⁻⁶

C
1.64×10⁻⁵

D
1.64×10⁻³

Solution
Question 10
1 / -0

Two moles of ammonia was introduced in an evacuated vessel of 1L capacity. At high temperature, the gas undergoes partial dissociation according to the equation:

2NH₃(g) ⇌ N₂(g) + 3H₂(g)

At equilibrium the concentration of ammonia was found to be 1mol. What is the value of K ?

A
3/4 = 0.75mol²L⁻²

B
3/2 = 1.5mol²L⁻²

C
27/16=1.7mol²L⁻²

D
27/64 = 0.42mol²L⁻²

Solution

Hence we have :

At equilibrium : [NH₃] = 2−2α = 1 or α = 1/2