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Extra! -100 27 1. Calculate Eº, AG, and K for the following reaction: Zn** (aq) +...
Calculate Eº, E, and AG for the following cell reactions (a) Mg(s) + Sn2+(aq) =Mg2+(aq) + Sn(s) where [Mg2+] = 0.040 M and [Sn2+] = 0.045 M 8° = 2.23 10 E = 2.23 AG=430390 (b) 3Zn(s) + 2Cr3+(aq) = 3Zn2+(aq) + 2Cr(s) where [Cr3+] = 0.040 M and [Zn2+] = 0.0065 M E° = 0.03 E = 0.0671 AG=-0.0389
What is the equilibrium constant for the following reaction at 298 K? 2 Ag+(aq) + 2 I-(aq) → I2(s) + 2 Ag(s) Eº = +0.265 V Group of answer choices 2.99 x 104 1.60 x 107 9.04 x 108 87.9 7.73 x 103 Using data from the reduction potential table below and the reaction 2 Ag(s) + Pt2+(aq) → Pt(s) + 2 Ag+(aq) Eº = 0.38 V calculate the standard reduction potential of the half-reaction Pt2+(aq) + 2 e- →...
Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) +Zn(s)Fe(s)+ Zn2 (aq) AG=-60.73 kJ/mol Calculate the standard cell potential, E for the reaction. V Ell Calculate the equilibrium constant, K, for the reaction. K =
Consider the following reaction and its AG at 25.00 °C. Fe2+ (aq) + Zn(s) Fe(s) + Zn2+ (aq) AG = -60.73 kJ/mol Calculate the standard cell potential, E , for the reaction. Ecell Calculate the equilibrium constant, K, for the reaction.
The equilibrium constant, K, for a redox reaction is related to the standard potential, Eº, by the equation In K = nFE° RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e), R (the gas constant) is equal to 8.314 J/(mol · K), and T is the Kelvin temperature. Standard reduction potentials Reduction half-reaction E° (V) Ag+ (aq) + e +Ag(s) 0.80 Cu²+ (aq) + 2e + Cu(s) 0.34...
For the following redox reaction at 25 ºC, Eº cell = 2.24 V. Calculate the equilibrium constant, K. Mg(s) + Pb 2+ (aq) → Mg 2+ (aq) + Pb(s)
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq)|Cu(s) (a) The oxidation half-reaction is clearly Zn(s) ® Zn** (aq) + 2 e. (b) The oxidation half-reaction is clearly Zn() Zn" (aq) +le. (C) The oxidation half-reaction could not be anything other than Cu(s) ® Cu (aq) +2 e. (d) It is obvious that the oxidation half-reaction is Zn(s) ® Cu(s). 5. Which of the following statements about the voltaic cell shown...
What is Eº for the cell Mn| Mn2+ (aq) || Ag+ (aq) | Ag? Standard Reduction Potentials E° (V) Ag+(aq) + e + Ag(s) +0.80 Mn2+(aq) + 2e Mn(s) -1.18 V 1 2 3 Х 1
Calculate the cell potential for the following reaction: Mg (s) + Ag₂SO₄ (aq) → 2 Ag (s) + MgSO₄ (aq) E° (Mg²⁺/Mg) = -2.37 V E° (Ag⁺/Ag) = 0.80 V
please answer in 10m 5. Balance each reaction, calculate the net Eº, and declare each reaction as being spontaneous or non- spontaneous. (9) a) Sn?' (aq) + Cr(s) → Sn(s) + Cr?" (aq) net Eº = b) Ag+ (aq) + Mn(s) Ag(s) + Mn2(aq) net Eº = c) Fe2(aq) + Cu(s) → Fe(s) + Cu?"(aq) net Eº =