From the Standard Potential Table in your general chemistry textbook: Which reaction has been chosen as the 'standard' against which every other reaction is measured?
A. 2H+ + 2e–H2
B. Li+ + e–Li
C. O2 + 4H+ + 4e–2H2O
D. F2 + 2e–2F–
E. H2 + 2e–2H–
is it A
A it is.
It's A
A is the correct answer!
A is right :)
To determine which reaction has been chosen as the 'standard' against which every other reaction is measured from the Standard Potential Table, we need to look for the reaction with the highest standard potential value. The standard potential is a measure of the tendency of a half-reaction to undergo reduction or oxidation under standard conditions.
Here are the standard potential values for each reaction:
A. 2H+ + 2e– → H2 E° = 0.00 V
B. Li+ + e– → Li E° = -3.04 V
C. O2 + 4H+ + 4e– → 2H2O E° = 1.23 V
D. F2 + 2e– → 2F– E° = 2.87 V
E. H2 + 2e– → 2H– E° = -2.25 V
As we can see, reaction D. F2 + 2e– → 2F– has the highest standard potential value of 2.87 V. Therefore, the answer is D. F2 + 2e– → 2F–.