7. The following system has Ecell = 0.8401 V at 1000 K: (10 pts) Ag(s) +...
Use the Nernst equation to calculate Ecell for each of the following cells. Ag(s)|Ag+( 0.34 M )||Cl−( 0.095 M )|Cl2(g, 0.50 bar )|Pt(s) Thank you for any help
19.03 pts Question 10 Use the standard reduction potenital to calculate equilibrium constants for the following reaction at 298.15 K. AgCl (s) Ag+ (aq) +Cl- (aq) Ag+ (aq) +Ag(s) E° = 0.7996 V AgCl(s) + e - Ag(s) + CH- (aq) E° = 0.22233 V O K=5.2 x 105 spontaneous O K = 3.8 x 10"nonspontaneous K - 1.7 x 10-10 nonspontaneous
StUP 7. (5 pts) The equilibrium constant for dissociation of silver chloride AgCl (s) Ag' (aq) + CI (aq) Is 1.8x1010 Find concentration of silver and chloride ions in saturated aqueous solution of silver chloride (10 pts) The equilibrium constant at certain temperature for 8 H2(g) +1:(g) 2 HI(g) is 55.17. If 10mole of hydrogen and 1.0 mole of iodine are placed in 0.5L flask, what is the equilibrium concentration of hydrogen iodide? (10 pts) Solid ammonium carbamate decomposes to...
A voltaic cell represented by the following cell diagram has Ecell= 1.409 V . Zn(s)|Zn2+(1.00M)||Ag+(saturated Ag2X)|Ag(s) What must be the Ksp of Ag2X? Use the following standard electrode potentials: Zn2+(aq) + 2e- →Zn(s) E° = -0.764 V Ag+(aq) + e- →Ag(s) E° = 0.799 V To enter your answer, multiply your Ksp by 1x109 then enter it to 2 decimal places.
9. (12 pts) Answer parts a-b for the following reaction: Hos?"(aq) + 2 Ag(s) = Hg () + 2 Agt(aq) a) Calculate the equilibrium constant at 37 °C. -> 310K - С. 2 46°.. - КТК - = -8.314 (310) Ink Ecele = Fired (reduced) - Ered (oxidized) (no need to flip signs!) E = pº In QC q=1.t 1 C = 1 A-s F = 96485 C/mole e R = 8.314 J/mole K or 0.082057 L.atm/mole K PV=nRT Ered...
Consider the following reaction and its AG at 25.00 °C. Mg(s) + Ni2+ (aq) Mg2+ (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, Ecell for the reaction. 2.11 V Enter numeric value Calculate the equilibrium constant, K, for the reaction. K= 3.30 x1071 Incorrect
7:32 Ksp.docx Write K, expression Set-up an ICE chart The initial concentration of Ag" is 0.100 M. Practice Problems: 1 , what is the molar solubility of BaF, at 25 C? K,= 1.0E-6 2. Determine which salt, CaCO, or Ag CO, is more soluble in water in units of moles per liter? K,-2.8 x 10 CaCO AgCO: K 8.1x 10 3. Calculate the molar solubility of AgCI in pure water. (AgC K-1.8 x 10 a. Calculate the solubility of AgCl...
1) Given the reaction Cd(s)+Ni2+(aq)------>Cd2+(aq)+Ni(s) Calculate the equilibrium constant (K). Ecell of +0.350 V and at 25.0 celsius 2)If 75.0mL of 0.195 M Hbr is combined with 75.0mL of 195M Ca(OH)2 at 25.0 celsius calculate the pH of this solution
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.
Consider the following Gibbs energies at 25 "C Substance Ag (aq) Cr(aq) AgCI(s) Br(aq) AgBr(s) 77.1 - 131.2 - 109.8 - 104.0 -96.9 (a) Calculate AG rn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl Number Number kJ mol (c) Calculate Δ3rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr Number Number kJ mol