If Fe2++2e-1 xrightarrow[]Fe; E° =-0.44V and Zn2++2e- xrightarrow[]Zn; E° =-0.76 V which of the following is the correct statement?

Question

If Fe2++2e-1 xrightarrow[]Fe; E° =-0.44V and Zn2++2e- xrightarrow[]Zn; E° =-0.76 V which of the following is the correct statement? (A) Fe is more electropositive (B) Zn is more electropositive (C) Zn is more electronegative (D) None of the above

Tardigrade Admin · Accepted Answer

The electropositive character of metals increases with the increasing tendency to give the electron. Hence, the metal which has low reduction potential will be more, electropositive. Here, the reduction potential of Fe is lesser than Zn hence Fe is more electropositive.

Q. If Fe2++2e−1​Fe; E∘=−0.44V and Zn2++2e−​Zn; E∘=−0.76V which of the following is the correct statement?

Fe is more electropositive

Zn is more electropositive

Zn is more electronegative

None of the above

The electropositive character of metals increases with the increasing tendency to give the electron. Hence, the metal which has low reduction potential will be more, electropositive. Here, the reduction potential of Fe is lesser than Zn hence Fe is more electropositive.

Q. If $F e^{2 +} + 2 e^{- 1} F e;$ $E^{\circ} = - 0.44 V$ and $Z n^{2 +} + 2 e^{-} Z n;$ $E^{\circ} = - 0.76 V$ which of the following is the correct statement?