A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at 25.0°C and each compartment has a volume of 219 mL. The cell delivers 0.25 A for 31.5 h. (a) How many grams of Cu are deposited? 4) 9.3 (b) What is the [Mg2+ ]? Assume constant volumes. 40.66826 X mol·L-1

A voltaic cell using Cu/Cu²+ and Sn/Sn²+ half-cells is set up at standard conditions, and each compartment has a volume of 345 mL. The cell delivers 0.17 A for 31.5 h. (a) How many grams of Cu(s) are deposited? 9.7 (b) What is the [Cu²+ ] remaining? 0.56

2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ EⓇ = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+]= 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CUSO4 solution? Cu²+ +ze--- Cu(s)

Balance the following redox reaction in aqueous basic solution: 3- NO3 (ag) + Fe(CN),- → NO(9) + Fe(CN)6' + Fe(CN)6 (aq) (ад)

I need help with all parts. Thanks

4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.

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)

Help with the following question Please round the answer to 3 sig figs

O ELECTROCHEMISTRY = Understanding concentration cells ODDOD 3/5 A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of MNO3 and the right half cell with a 150. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? Oleft right ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.