[shawen]

Identify the element oxidized and reduced in these redox reactions. Then calculate the standard cell
potential (E°cell) for each. Would each react spontaneously as written (+ E°) or in the reverse(– E°)?

a. 2 NaCl + Co –––> CoCl2 + 2 Na
 
b. Cu(NO3)2 + Ni –––> Ni(NO3)2 + Cu

c. I2 + 2 Fe+2 –––> 2 I– + 2 Fe+3
(For: Fe+3 + e– —> Fe+2 : E°red = +0.77 V)

d. 2 Cr+2 + Cu+2 –––> 2 Cr+3 + Cu
(For: Cr+3 + e– –––> Cr+2 : E°red = – 0.41)

could anyone please answer question
thanks so much

[billnotgatez]

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[IonNick]

^
First you need to determine oxidation states for each of the atoms in each of the reagents and products and then determine which atoms are gaining or losing electrons. Then split the overall reaction into half reactions, one for oxidation and one for reduction. Then look at the reduction potentials for each of the reaction to determine the standard cell potential. If the potential is positive then the cell is galvanic and also spontaneous.