Equilibrium Constant and Reaction Quotient
This worksheet covers the concepts of equilibrium constant (Kc, Kp) and reaction quotient (Qc, Qp) for Grade 11 Chemistry students.
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Equilibrium Constant and Reaction Quotient
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Read each question carefully and provide your answers in the space provided. Show all your work for calculations.
1. Which of the following statements is TRUE regarding the equilibrium constant (Kc)?
It changes with concentration.
It changes with temperature.
It changes with the addition of a catalyst.
It changes with pressure.
2. For the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), which expression represents Kp?
Kp = [SO₃]² / ([SO₂]²[O₂])
Kp = (P(SO₃))² / ((P(SO₂))² P(O₂))
Kp = (P(SO₂))² P(O₂) / (P(SO₃))²
Kp = ([SO₂]²[O₂]) / [SO₃]²
3. When the reaction quotient (Qc) is less than the equilibrium constant (Kc), the reaction will proceed in the direction to reach equilibrium.
4. A large value of Kc indicates that the equilibrium lies predominantly towards the .
5. Consider the reversible reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Write the expression for the equilibrium constant (Kc).
6. At a certain temperature, the equilibrium constant (Kc) for the reaction H₂(g) + I₂(g) ⇌ 2HI(g) is 50.0. If, at a particular moment, the concentrations are [H₂] = 0.10 M, [I₂] = 0.20 M, and [HI] = 1.0 M, calculate the reaction quotient (Qc) and predict the direction the reaction will shift to reach equilibrium.
7. For a heterogeneous equilibrium, the concentrations of pure solids and liquids are included in the equilibrium constant expression.
True
False
Match each term on the left with its definition on the right.
8. Equilibrium Constant
a. Ratio of products to reactants at any given time
9. Reaction Quotient
b. A state where forward and reverse reaction rates are equal
10. Chemical Equilibrium
c. Ratio of products to reactants at equilibrium
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