Home
Class 11
CHEMISTRY
(A) Absolute electrode potential can be ...

(A) Absolute electrode potential can be easily measured by using vacuum tube voltmeter.
(R ) Oxidation or reduction cannot take place alone,

A

If both (A) and (R ) are true. and (R ) is the correct explanation of (A).

B

If both (A) und (R ) are true, but (R ) is not the correct explanation of (A).

C

lf (A) and (R ) is false.

D

lf (A) and (R )are both false.

Text Solution

Verified by Experts

The correct Answer is:
D
Promotional Banner

Topper's Solved these Questions

  • OXIDATION AND REDUCTION (REDOX REACTIONS)

    OP TANDON|Exercise MATRIX MATCHING|6 Videos
  • OXIDATION AND REDUCTION (REDOX REACTIONS)

    OP TANDON|Exercise INTEGER TYPE|11 Videos
  • OXIDATION AND REDUCTION (REDOX REACTIONS)

    OP TANDON|Exercise STEP II|7 Videos
  • MISCELLANEOUS (TOPICS OF GENERAL INTEREST)

    OP TANDON|Exercise SET-VI: Problems on graphical aptitude|53 Videos
  • POLYMERS

    OP TANDON|Exercise PASSAGE 3|5 Videos

Similar Questions

Explore conceptually related problems

Can absolute electrode potential of an electrode be measured?

Statement-2: Absolute value of E_(red)^(0) of an electrode cannote be determined. Statement-2: Neither oxidation nor reduction can take place alone.

Statement-1: Absolute value of E_("red")^(@) of an electrode cannot be determined. statement-2: Neither oxidation nor reduction can take place alone.

Statement-I: Absolute value of E_(red)^(0) of an electrode cannot be determined. Because Statement-II: Neither oxidation nor reduction can take place alone.

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 : Absolute value of E_(ced)^@ of an electrode cannot be determinde . Neigher oxdation nor reduction can take place alone.

Assertion(A): The absolute value of the electrode potential cannot be determined experimentally Reason (R): The electrode potentials are generally determined with respect to standard hydrogen electrodes.

STATEMENT-1: In the reaction : Cl_(2)+ OH^(-) to Cl^(-) + ClO_(4)^(-) chlorine is oxidised only STATEMENT-2: Oxidation and reduction cannot take place alone.