chemistry : class11 Homogeneous Equilibrium : Equilibrium in chemical processes : Equilibrium MCQ Questions and Answers
Practice important
Homogeneous Equilibrium
MCQ questions and answers.
Page 2
of
2
|
20
MCQ Questions
1. What is meant by homogeneous equilibrium?
A.
Equilibrium between solids only
B.
Equilibrium in which all reacting species are in the same phase
C.
Equilibrium between a solid and a liquid
D.
Equilibrium involving only a catalyst
Correct Answer:
Equilibrium in which all reacting species are in the same phase
Explanation:
Homogeneous equilibrium occurs when all reactants and products are present in the same physical phase, such as all gases or all aqueous species.
2. Which reaction represents a homogeneous gaseous equilibrium?
A.
N2(g) + 3H2(g) ⇌ 2NH3(g)
B.
CaCO3(s) ⇌ CaO(s) + CO2(g)
C.
AgCl(s) ⇌ Ag+(aq) + Cl−(aq)
D.
Ice(s) ⇌ Water(l)
Correct Answer:
N2(g) + 3H2(g) ⇌ 2NH3(g)
Explanation:
All the species in the ammonia formation reaction are gases, so it is a homogeneous gaseous equilibrium.
3. For the homogeneous equilibrium H2(g) + I2(g) ⇌ 2HI(g), which expression represents Kc?
A.
[H2][I2]/[HI]2
B.
[HI]2/[H2][I2]
C.
[HI]/[H2][I2]
D.
[H2][I2][HI]2
Correct Answer:
[HI]2/[H2][I2]
Explanation:
For a reaction, the equilibrium constant in concentration form is the product concentration raised to its coefficient divided by the reactant concentrations raised to their coefficients.
4. At chemical equilibrium in a homogeneous reaction, what happens to the forward and reverse reaction rates?
A.
Both reactions stop completely
B.
The forward reaction is faster than the reverse reaction
C.
The reverse reaction is faster than the forward reaction
D.
The forward and reverse reaction rates become equal
Correct Answer:
The forward and reverse reaction rates become equal
Explanation:
Homogeneous chemical equilibrium is dynamic. The forward and reverse reactions continue, but their rates are equal, so the concentrations remain constant.
5. Which statement is true about the concentrations of reactants and products at homogeneous equilibrium?
A.
They become equal
B.
They remain constant with time
C.
They become zero
D.
They change continuously in one direction
Correct Answer:
They remain constant with time
Explanation:
At homogeneous equilibrium, equal forward and reverse reaction rates keep the concentrations of all species constant, although the reactions continue.
6. For the equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g), which is the correct Kc expression?
A.
[SO2]2[O2]/[SO3]2
B.
[SO3]2/[SO2]2[O2]
C.
[SO3]/[SO2][O2]
D.
[SO2][O2]/[SO3]
Correct Answer:
[SO3]2/[SO2]2[O2]
Explanation:
The equilibrium expression places products over reactants and uses the stoichiometric coefficients as powers.
7. Which of the following is a homogeneous aqueous equilibrium?
Explanation:
In this equilibrium, acetic acid, hydrogen ions, and acetate ions are all present in the aqueous phase, making it homogeneous.
8. What does the double arrow (⇌) in a homogeneous equilibrium reaction indicate?
A.
The reaction occurs only in the forward direction
B.
The reaction is irreversible
C.
The forward and reverse reactions can occur
D.
The reaction does not involve products
Correct Answer:
The forward and reverse reactions can occur
Explanation:
The double arrow shows that a homogeneous reaction is reversible and can reach a state of dynamic equilibrium.
9. For the homogeneous equilibrium N2(g) + 3H2(g) ⇌ 2NH3(g), which species is a product?
A.
N2(g)
B.
H2(g)
C.
NH3(g)
D.
N2(g) and H2(g)
Correct Answer:
NH3(g)
Explanation:
In the reaction, nitrogen and hydrogen are reactants, while ammonia is the product formed at homogeneous equilibrium.
10. What is the effect of a catalyst on a homogeneous equilibrium system?
A.
It changes the equilibrium constant
B.
It shifts equilibrium only toward products
C.
It shifts equilibrium only toward reactants
D.
It helps the system reach equilibrium faster
Correct Answer:
It helps the system reach equilibrium faster
Explanation:
A catalyst speeds up both the forward and reverse reactions equally. Therefore, it does not change the position of homogeneous equilibrium but helps reach it more quickly.