The standard reduction potentials of Cr³⁺/Cr , Cd²⁺/Cd , Co²⁺/Co , and Sn²⁺/Sn are -0.74 V , -0.40 V , -0.28 V , and -0.14 V respectively. Based on these values, which of the following reactions is spontaneous under standard conditions?

Step-by-step solution

For a reaction to be spontaneous under standard conditions, the standard cell potential E^ _ cell must be positive. E^ _ cell = E^ _ cathode - E^ _ anode A metal with a more negative standard reduction potential acts as the anode (undergoes oxidation) and can reduce the ion of a metal with a less negative standard reduction potential. The given standard reduction potentials are: E^ (Cr³⁺/Cr) = -0.74 V E^ (Cd²⁺/Cd) = -0.40 V E^ (Co²⁺/Co) = -0.28 V E^ (Sn²⁺/Sn) = -0.14 V The reducing power of the metals follows the o