Calculate the equilibrium constant for the reaction 2 Cu+⇄Cu2++ Cu(s)usingstandard potential data for reactions: Cu+ + e- ----->Cu(s) Eo= + 0.52 V Cu2+ + 2e-    ------> Cu (s)Eo= + 0.34 V

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Fe*(aq) + Ni(s)- →2FE?*(aq) + Ni²+(aq) 2+ Answer: kJ K for this reaction would be than one.

Consider the following reaction and standard reduction potential data. 2Ag (aq) + Cu(s) 2Ag(s) + Cu*"(aq) Half reaction E°(V) Ag (aq) +eAg(s) 0.80 Cu2"(aq) + 2e → Cu(s) 0.34 a. As written, is the Keg of the reaction shown above greater than 1 or less than 17 (Select] b. Which species is the reducing agent? [Select ] c. Suppose a voltaic cell was constructed using a Cu and Ag electrode (pictured below). The Cu electrode was placed in a 0.01 M solution of Cu(NO;)2, and the Ag electrode was placed in a 1.00 M solution of AGNO3. What is the Ecell for this voltaic cell? Assume the temperature is 298 K. Also NO; is a spectator ion. ( Select ) Voltmeter Ag Cu sat bridge AgNO= 1.00 M -0.01 M >

Given the standard reduction potentials: Zn2*(aq) + 2e- Zn(s) Ag*(aq) + e + Ag(s) E°=-0.76 V E°= 0.80 V Which species is the best oxidizing agent? Ag(s) O Ag*(aq) O Zn(s) O Zn2*(aq)

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction ele 2Cr3+, *(aq) + 3Cu(s)–→2Cr(s) + 3Cu²*(aq) Answer: kJ K for this reaction would b v than one. greater less

Please don't provid handwritten solution

Find the equilibrium constant Kc for this reaction below:Cu(s) + 2 Pe+(aq) <-> Cu2+(aq) + 2 Pe(s)