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Calculate the Ecell for the following reaction? Zn(s)  +  Fe2+(aq, 0.1 M)  ↔  Zn2+(aq, 1.9 M)  +  Fe(s) Use:  Zn2+(aq)  +  2e-  ↔  Zn(s)  Ecell = -0.76 V Fe2+(aq)  = 2e-  ↔  Fe(s)  Ecell = -0.447 V

Predict the products for the following reaction Zn(s)  +  2H+(aq)   →   

Acidity of H-halogen is increasing down the group. Which of the following statement best describes this phenomenon?

Based on the answer you received for question 23, determine whether the cell is spontaneous or non-spontaneous Pb2+(aq)  +  2e-  = Pb(s)       Ecell = -0.13 V Ca2+(aq)  +  2e-  = Ca(s)     Ecell= -2.87 V Choose (A) or (B)

During a redox reaction

Which of the following is most likely to act as a Lewis acid?

Consider the following half-cell reactions: Zn2+(aq)  +  2e-  ↔  Zn(s)  Ecell = -0.76 V Cu2+(aq)  +  2e-  ↔  Cu(s)  Ecell = +0.34 V Identify the species (element or ion) that is getting oxidized Hint: The half-cell with the highest positive potential gets reduced

An aqueous solution is made by mixing 15% NH3 with DI water. Identify the acidic component in the newly formed solution.

Identify the oxidizing species in the following reaction Ag+(aq)   +  Al(s)  →  3Ag(s)  +  Al3+(aq)

Consider the reaction shown below: Ag+(aq) + 2NH3(aq) →  Ag(NH3)2+(aq) Identify the correct answer