Given that E^o_{K^{+}/K} = -2.93 V,E^o_{Fe^{ | vedclass

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(B) reducing agent is a substance that undergoes oxidation (loses electrons). The strength of a reducing agent is determined by its standard oxidation

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$K_{(s)}$

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(B) reducing agent is a substance that undergoes oxidation (loses electrons). The strength of a reducing agent is determined by its standard oxidation potential,which is the negative of its standard reduction potential $(E^o_{ox} = -E^o_{red})$.Comparing the standard reduction potentials $(E^o_{red})$:$E^o_{K^{+}/K} = -2.93 \ V$$E^o_{Zn^{2+}/Zn} = -0.76 \ V$$E^o_{Fe^{2+}/Fe} = -0.44 \ V$$E^o_{Cu^{2+}/Cu} = 0.34 \ V$The species with the most negative standard reduction potential is the strongest reducing agent because it has the highest tendency to lose electrons.Since $E^o_{K^{+}/K} = -2.93 \ V$ is the most negative value,$K_{(s)}$ is the strongest reducing agent.

Given that $E^o_{K^{+}/K} = -2.93 \ V$,$E^o_{Fe^{2+}/Fe} = -0.44 \ V$,$E^o_{Zn^{2+}/Zn} = -0.76 \ V$,and $E^o_{Cu^{2+}/Cu} = 0.34 \ V$. Based on this data,which of the following is the strongest reducing agent?

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