Home
Class 12
CHEMISTRY
Assertion : If E^(@) value for reaction ...

Assertion : If `E^(@)` value for reaction `Ag^(+)+e^(-) to Ag` is `0.80" V"`, then the value of reverse reaction will be `1.60" V"`.
Reason : If concentration of `Ag^(+)` ions is doubled, the electrode potential will be also doubled.

A

If both assertion and reason are correct and reason is correct explanation for assertion.

B

If both assertion and reason are correct but reason is not correct explanation for assertion.

C

If assertion is correct but reason is incorrect.

D

If assertion and reason both are incorrect.

Text Solution

Verified by Experts

The correct Answer is:
D
(d) Correct reason : Standard reduction potential (`E^(@)`) of an electrode has fixed value.
Correct assertion : Effect of concentration is studied by Nernst equation.
Promotional Banner

Topper's Solved these Questions

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise COMPLETION QUESTION|2 Videos

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise NCERT In-Text Questions|9 Videos

  • ALDEHYDES AND KETONES

    DINESH PUBLICATION|Exercise Interger|5 Videos

Similar Questions

Explore conceptually related problems

The questions consist of two atatements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses : If standard reduction potential for the reaction Ag^+ = 2e^- Ag is 0. 80 volt, then for the raction 2 Ag^+ = 2e^- = 2e^- 2Ag , it will be 1, 60 volt . If concentration of Ag^+ ions is doubled , the standard electrode potential is also doubled.

In a cell reaction, Cu_((s))+ 2Ag_((aq))^(+) to Cu_((aq))^(2+) + 2Ag_((s)) E_"cell"^@ =+0.46 V . If the concentration of Cu^(2+) ions is doubled then E_"cell"^@ will be

(a) Write the anode and cathode reactions and the overall reaction occuring in a lead storage battery. (b) A copper - silver cell is set up. The copper ion concentrations is 0.10 M. The concentration of silver ion is not known. The cell potential when measured was 0.422 V. Determine the concentration of silver ions in the cell. Given " "E^(@)Ag^(+)//Ag=+0.80 V,E^(@)Cu^(2+)//Cu=+0.34 V

Calculate the following cell reaction cell at 298 K. 2Ag^(+)+Cd to 2Ag+Cd^(2+) E^(@) for Ag^(+)//Ag and Cd^(2+)//Cd are 0.80 V and -0.40 V respectively. E^(@) for Ag^(+)//Ag and Cd^(2+)//Cd are 0.80 V and -0.40 V respectively. (i) Write the cell representation. (ii) What will be the emf of the cell if the concentration of Cd^(2+) is 0.1 M ? (iii) Will the cell work spontaneously for the condition given above ?

The standard electrode potential (reduction) of Ag^(+)|Ag is 0.800 V at 25^(@)C . Its electrode potential in a solution containing 10^(-3)M ion of Ag^(+) ions is:-