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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)
When [Co(H₂O)₆]²⁺ and Cl¯ ions are in equilibrium in a solution, which of the following factors will cause a shift in the equilibrium towards the formation of more [Co(H₂O)₆]²⁺ ions?
Decreasing the temperature of the solution
Increasing the concentration of [Co(H
2
O)₆]²⁺ ions
Increasing the concentration of Cl
–
ions
Adding a substance that removes Cl
–
ions
2)
Equilibrium is best defined as
Stage where the rate of forward reaction is equal to that of backward reaction
Stage where the concentration of reactants is less than that of products
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?
Can be physical or chemical
Dynamic nature
All of these
Requires a closed system
4)
What is the colour of [Co(H₂O)₆]²⁺ ions?
Blue
Pink
Light blue
Purple
5)
Equilibrium can be attained in
All types of system
Closed system
Open system
Isolated 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]²⁻
[CoCl₄]¹⁺
[CoCl₄]
[CoCl₄]²⁺
7)
Le Chatelier’s principle is applicable to:
Only physical equilibrium
Only homogeneous chemical reversible reactions
All systems, chemical or physical in equilibrium
Only heterogeneous chemical reversible reactions
8)
Which of the following is not a characteristic of equilibrium?
Equilibrium occurs in reversible conditions
Rate is equal in both directions
Measurable quantities are constant at equilibrium
Equilibrium occurs only in open vessels at constant temperature
9)
What is the coordination number of the central cobalt ion in the complex [Co(H₂O)₆]²⁺ ?
2
4
6
3
10)
According to Le Chatelier’s principle, what happens when concentrated HCl is added?
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 right
Increases the chloride ion concentration and causing the position of equilibrium will move to the left