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Study the Shift in Equilibrium between [Co(H₂O)₆] ²⁺ and Cl⁻ ions
Study the Shift in Equilibrium between [Co(H₂O)₆] ²⁺ and Cl⁻ ions
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1)
Which one of the following is CORRECT regarding chemical equilibrium?
Equilibrium constant depends on the initial concentration of the reactant
Equilibrium is achieved only when temperature of the reaction is increased
Equilibrium is achieved only when pressure of the reaction is decreased
Equilibrium is achieved when forward reaction rate equals reverse reaction rate
2)
Equilibrium is best defined as
Stage where the concentration of reactants is less than that of products
Stage where the rate of forward reaction is equal to that of backward reaction
Stage where concentration of reactants is equal to that of products
Stage where the concentration of reactants is less than that of products
3)
Which of the following characterizes Equilibrium?
Requires a closed system
Dynamic nature
All of these
Can be physical or chemical
4)
What is the colour of [Co(H₂O)₆]²⁺ ions?
Purple
Light blue
Pink
Blue
5)
Equilibrium can be attained in
All types of system
Open system
Isolated system
Closed system
6)
What is the formula of the complex ion formed when a solution containing [Co(H₂O)₆]²⁺ ions is treated with hydrochloric acid?
[CoCl₄]¹⁺
[CoCl₄]²⁻
[CoCl₄]
[CoCl₄]²⁺
7)
Le Chatelier’s principle is applicable to:
All systems, chemical or physical in equilibrium
Only physical equilibrium
Only homogeneous chemical reversible reactions
Only heterogeneous chemical reversible reactions
8)
Which of the following is not a characteristic of equilibrium?
Equilibrium occurs in reversible conditions
Measurable quantities are constant at equilibrium
Equilibrium occurs only in open vessels at constant temperature
Rate is equal in both directions
9)
The reaction [Co (H₂O)₆]²⁺(aq) + 4Cl⁻(aq) → [CoCl₄]²⁻(aq) + 6H₂O(l) is
Biological
Isothermic
Exothermic
Endothermic
10)
According to Le Chatelier’s principle, what happens when concentrated HCl is added?
Increases the chloride ion concentration and causing the position of equilibrium will move to the right
Decreases the chloride ion concentration and causing the position of equilibrium will move to the left
Decreases the chloride ion concentration and causing the position of equilibrium will move to the right
Increases the chloride ion concentration and causing the position of equilibrium will move to the left
