A student was asked to answer the following: Calculate the time (in sec) that is required to plate out 0.702g of aluminum when a current of 2.10A is applied to 5.0L of a 0.75M AI(NO3)3 solution. The molar mass of copper is 26.98g/mol. The student set up the following calculation: mol mol 2.10A* *5.0L * 96485C 0.75 mol 0.702g Identify twO Ro spocific

Consider the cell: Cu | Cu2+(aq, 0.5 M)|| Ag2+(aq, 5.0 M) | Ag Write the balanced net chemical reaction.

What is the net reaction for the cell?  Is it .44V or .22V?

Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)   It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information)   (Show your work)                                                                                        2H+ (aq) + 2e- → H2 (g)          Eºred = 0.000 V   Zn2+ (aq) + 2e- → Zn(s)         Eºred = -0.762 V

A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative

(19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) → Cr³+ (aq) + Cut (aq) If the cell is operating at 25°C, what is the value of the equilibrium constant (Keq)? (A) 1.41 x 10¹1 1.19 x 1018 5.53 x 105 2.79 x 1033 1.81 x 10-6 (B) (C) (D) (E)

Consider the following cell reaction: Ni(s) + 2 H*(? M). Ni?*(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.118 volts, what is the pH of the hydrogen electrode? pH =