Use the information in the equation below and the Delta G degree below Delta d_f

Question

Use the information in the equation below and the Delta G degree below Delta d_f degree for NH_3; and K_p for NH_3 at 25 degree C N_2(g) + 3 H_2(g) 2 NH_3 (g), Delta G degree = -31.0 kJ Consider the galvanic cell that uses the reaction 2 Ag^+(aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell. For the following cell, write a balanced equation for the cell reaction and calculate E degree and Delta G degree at 25 degree C: Pt(s) |H_2(1.0atm)| H^+(1.00M) |Cu^2+|(1.00M)|Cu(s) Calculate the standard cell potential, E degree, for each of the following reactions and predict whether or not reaction will take place spontaneously under standard conditions: Al(s) + Cr^3+(aq) rightarrow Al^3+ (aq) + Cr(s) 2 Ni(5) + 6 H^+(aq) rightarrow 2 Ni^2+(aq) + 3 H_2(g) O_2(g) + 2 Fe(s) + 4 H^+(ag) rightarrow 2 Fe^2+(aq) + 2 H_2O Consider the following galvanic cell that uses the reaction. Sn(s) + Sn^4+(aq) rightarrow 2 Sn^2+(aq) What is the potential of a cell at 25 X that has the following ion concentrations? [Sn^4+] = 0.50 M, l Sn^2+] = 0.20 M What is the pH of the solution in the anode compartment of the following cell if the measured cell potential at 25 degree C is 0.28 V: Pt(s)|H_2(1 atm)|H^+(times M|| Pb^2+ (1 M)|Pb(s)?

Explanation / Answer

5. N2 (g) + 3 H2 (g) 2 NH3 (g) G0 = -31KJ

a) Calculate G0f NH3

G0f for N2 and H2 is 0

G0 = [2G0 f(NH3 (g))] - [1G0 f(N2 (g)) + 3Gf(H2 (g))]

31.0KJ = [2G0f (NH3 (g))] - [1(0) + 3(0)]

[2G0f (NH3 (g))] = 31.0KJ

G0f (NH3 (g) =   -31 kJ/2 = 15.5KJ

b)

KP for NH3 at 250C

KP = e^- G0/RT

G0 = -15.5KJ = -15500 J

R = 8.314 J/mol.K

T = 25 + 273 = 298 K

First calculate

- G0/RT = - (-15500J)/8.314 J/mol.K x 298K

              = 6.25

KP = e^6.25

KP = 514.01

    = 5.14 x 10^2

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