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Given equation: K2CrO4(aq)+2Ag(s) +FeCl3(aq) —> Ag2CrO4(s) + 2FeCl2(aq) +2KCl (aq) Delta G = -62.5 kJ If...
1. Write the net ionic equation (has all the chemistry) for the following balanced reaction K2CrO4(aq) + 2 Ag(s) + 2 FeCl3(aq) → Ag2CrO4(s) + 2 FeCl2(aq) + 2 KCl(aq)
Question 9 Calculate AGⓇ for the reaction, 2A (g) + B2 (9) =72AB (9) given that at 120°C the equilibrium constant of the reaction is 3.21x105 -35.76 KJ/mol -414.30 J/mol None of these -41.43 KJ/mol -41.43 J/mol ving to another question will save Question 7 Calculate AGⓇ for the formation of ammonia, N2 (g) + 3H2(g)=2NH3(g) given that at 25°C the equilibrium constant of the reaction is 5.34x105 -32.7 KJ/mol 25.73 KJ/mol None of these 13.19 KJ/mol -32,700 KJ/mol Question...
Consider the following balanced equation: 16HCl(aq) + 2KMnO4(aq) → 5Cl2(g) + 8H2O(l) + 2KCl(s) + 2MnCl2(aq) If 8.53×102 grams of HCl(aq) reacts with an excess of KMnO4(aq), and the percent yield is 72.6%, how many grams of KCl(s) will actually be produced? 9.13×102 g 1.58×102 g 8.82×102 g 4.38×102 g 9.33×102 g
For the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) H° = -7.4 kJ and S° = 107.9 J/K The equilibrium constant for this reaction at 315.0 K is Assume that H° and S° are independent of temperature.
Calculate the cell potential (Ecell) and Gibbs Free Energy (Delta G) for the reaction (2Ag+ (aq) + Fe (s) -> Fe2+ (aq) + 2Ag (s) ) under these conditions: a 250mL beaker of 1.0mol Fe metal electrode and 0.10 moles of Fe 2+; and a second 250mL beaker of 2.0 moles Ag metal electrode ad 0.50 moles of Ag+. E naught of the cell= 1.21 V.
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
For the reaction Fe(s) + 2HCl(aq) FeCl2(5) + H2(g) AH° = -7.4 kJ and AS° = 107.9 J/K The equilibrium constant for this reaction at 281.0 K is Assume that AHº and ASº are independent of temperature.
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
Calculate Delta G^Compositefunction and K at 25 degree C for the reaction Cu_(s) + 2Ag^+(1.0M) doubleheadarrow Cu^2+ (1.0 M) +2Ag_(s)
Calculate the Entropy of the reaction equilibrium between 2NO2 - N2O4 given the equation: Delta G = Delta H - T Delta S where: Enthalpy = -47.5 Kj/mol Gibbs free energy = -3.59 Kj/mol Temperature = 298K