Complete the following chemical equations :
(i) MnO₄⁻(aq) + S₂O₃²⁻(aq) + H₂O(l) →
(ii) Cr₂O₇²⁻(aq) + Fe²⁺(aq) + H⁺(aq) →
Complete the following reactions—
(i) Cr₂O₇²⁻ + 6Fe²⁺ + 14H⁺ →
(ii) 2CrO₄²⁻ + 2H⁺ →
(iii) 2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺ →
Assign the reason for the following :
Copper (I) ion is not known in aqueous solution.
How would you account for the following ? Many of the transition elements are known to form interstitial compounds.
What are the transition elements ? Write two characteristics of the transition elements.
Write the preparation of following :
(i) KMnO₄ from K₂MnO₄
(ii) Na₂CrO₄ from FeCr₂O₄
(iii) Cr₂O₇²⁻ from CrO₄²⁻
Explain the following observation :
Most of the transition metal ions exhibit characteristic colour in aqueous solution.
State Raoult’s law for a solution containing nonvolatile solute. What type of deviation from Raoult’s law is shown by a solution of chloroform and acetone and why?
Explain the solubility rule “like dissolves like” in terms of intermolecular forces that exist in solutions.
Calculate the molality of ethanol solution in which the mole fraction of water is 0.88.
What is meant by elevation in boiling point? Why is it a colligative property?
What is meant by positive deviations from Raoult’s law ? Give an example. What is the sign of H for positive deviation ?
Following reactions can occur at cathode during the electrolysis of aqueous silver nitrate solution using Pt electrodes:
Explain why :
(i) E° for Mn³⁺/Mn²⁺ couple is more positive than that for Fe³⁺/Fe²⁺. (At. Nos. Mn = 25, Fe = 26).
(ii) Ce³⁺ can be easily oxidized to Ce⁴⁺. (At. No.Ce = 58).