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What is the value of ΔGo in kJ at 25 oC for the reaction between the...

What is the value of ΔGo in kJ at 25 oC for the reaction between the pair: Cu(s) and Cr3+(aq) to give Cr(s) and Cu2+(aq) Use the reduction potentials for Cr3+(aq) is -0.74 V and for Cu2+(aq) is +0.34 V. Give your answer using E-notation with ONE decimal place (e.g., 2.1 x 10-2 would be 2.1E-2; and 2.12 x 10-2 would also be 2.1E-2.). Do NOT include spaces, units, punctuation or anything else silly

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Answer #1

Ans. dG0 = 4.50E2

Step 1: The net reaction can be written as the sum of following two half-reactions: Oxidation-half 3 Cu(s) Reduction-half: 2 Cr (aq) 6 e Net Reaction 3 Cu(s) 2 Cr3+(aq) 3 Cu2+(aq)2 Cr(s) 3 Cu (a 6 e >2 Cr(s) 0.744 V -Equation 1 number of electrons transferred Steps for Writing the coupled REDOX Reaction: I. Write the oxidation-half reaction. Since the standard redox potential (E are given for reduction (gain of e) in standard redox-potential table, the oxidation-half reduction reaction is reverse of its standard redox Rxn. # When a reaction is reversed, the sign of its EU is reversed, too. The superscript E° represents reverse of standard redox potential II. Write the reduction-half reaction as such. No need of changing the sign of of its E. Where, n F Faradays constan96.485 kJ mol1 v-1 # Putting the values in equation 1- ΔGo--6 x 96.485 kJ mol-1 V-1x AG 450.39 -0.778 V Add the E values of two half-reactions WITHOUT changing their sign (because it has already been done in step

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