Home
Class 12
CHEMISTRY
The standard potential of the following ...

The standard potential of the following cell is 0.23 V at `15^(@)C` and `0.21V` at `35^(@)C`.`Pt|H_(2) |HCl(aq) |Agcl (s)|g(s)`
(i) write the cell reaction .
(ii) Calculate `DeltaH^(@)` and `DeltaS^(@)` for the cell reaction by assuming that these quantities remain unchanged in the range `15^(@)C` to `35^(@)C`.
(iii) calculate the solubility of `AgCl` in water at `25^(@)C`.
Give , the standard reduction potential of the `(Ag^(+)(aq) //Ag(s)` is 0.80 V at `25^(@) C`.

Text Solution

AI Generated Solution

To solve the given problem step by step, we will break it down into three parts as specified in the question. ### Part (i): Write the cell reaction. 1. **Identify the half-reactions:** - At the anode (oxidation): \[ \frac{1}{2} H_2 \rightarrow H^+ + e^- ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (SECTION - I) (Subjective Type Question)|12 Videos

  • COORDINATION COMPOUNDS

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (Section-J Aakash Challenger Questions )|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGNMENT (SECTION-D) (Assertion - Reason Type Questions)|4 Videos

Similar Questions

Explore conceptually related problems

The standard potential of the following cell is 0.23V at 15^(@)C and 0.21V at 35^(@)C: Pt|H_(2(g)|HCl(aq)|AgCl(s)|Ag(s) a. Write the cell reaction. b. Calculate DeltaH^(c-) and DeltaS^(c-) for the cell reaction by assuming that these quantities remain unchanged in the range 15^(@)C to 35^(@)C c. Calculate the solubility of AgCl in water at 25^(@)C . Given : The standard reduction potential of Ag^(o+)(aq)|Ag(s) is 0.80V at 25^(@)C .

The EMF of the following cellis 1.05V at 25^(@)C: Pt,H_(2)(g)(1.0 atm)|NaOH(0.1m),NaCl(0.1M)|AgCl(s),Ag(s) a. Write the cell reaction, b. Calculate pK_(w) of water.

The EMF of the following cellis 1.05V at 25^(@)C: Pt,H_(2)(g)(1.0 atm)|NaOH(0.1m),NaCl(0.1M)|AgCl(s),Ag(s) Write the cell reaction.

For the cell Zn|ZnCl_(2)(m)|AgCl,E is 1.24V at 25^(@)C and 1.260V at 35^(@)C of m=10^(-3) . Write down the cell reaction and calculate DeltaG, DeltaH, and DeltaS at 25^(@)C .

The emf of the following cell is 0.256 V at 25^@C and 0.2595 V at 35^@C. Calculate heat of reaction taking place at 25^@C. Pt(H_(2))|HCl(aq)||AgCl|Ag

Calculate the standard potential of the cell ,If the standard electrode potentials of Zn^(2+)//Zn and Ag^(+) //Ag are -0.763 V and + 0.799 V respectively .

The EMF of Westron standard cell is 1.0153 at 20^(@)C and 1.01807 at 25^(@)C . Calculate DeltaG,DeltaH, and Delta S for the cell reaction at 25^(@)C .

The standard potential of a cell using the reaction +3HgO(s)+2(overset(c-)(O)H) (aq) is 0.489V at 25^(@)C . What is the equilibrium constant of the reaction ?

Calculate the emf of the following cell at 25^(@)C Ag(s)|AgNO_(3) (0.01 M)||AgNO_(3) (0.05 M)|Ag (s)

The standard emf of the cell, Cd(s) |CdCI_(2) (aq) (0.1M)||AgCI(s)|Ag(s) in which the cell reaction is Cd(s) +2AgCI(s) rarr 2Ag(s) +Cd^(2+) (aq) is 0.6915 V at 0^(@)C and 0.6753V at 25^(@)C . The DeltaH of the reaction at 25^(@)C is,-

Home
Profile