The equilibrium constant for the reaction,
2Fe3+ (aq) + Hg22+(aq) 2Fe2+ (aq) + 2Hg2+ is Kc = 9.1 x 10-6 @298K
a. What is ΔGo at this temperature?
b. If reactants and products in their standard state concentrations (1M) are mixed, in which direction does the reaction proceed? Provide a numerical justification for your response.
c. Calculate ΔG when [Fe3+] = 0.20 M, [Hg22+] = 0.010 M, [Fe2+] = 0.010 M, and [Hg2+] = 0.025 M. In which direction will the reaction proceed to achieve equilibrium? Provide equation and values used in calculating ΔG.
Please show all work and provide equations used. Please use correct significant figures and correct units in answers.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
temp is : 298K QUESTION 9 Please show all work. For full credit provide equations used. Please use correct significant figures and correct units in answers. The equilibrium constant for the reaction, 2Fe3+ (aq) + Hg22+ (aq) = 2Fe2+ (aq) + 2Hg2+ is Kc = 9.1 x 10-6 @298K a. What is AGO at this temperature? b. If reactants and products in their standard state concentrations (1M) are mixed, in which direction does the reaction proceed? Provide a numerical justification...
Please show all work. Provide equations used for full credit. Please use correct significant figures and correct units in answers. The reaction, 2NOBr(g) + 2NO(g) + Br2(8) has an equilibrium constant, K = 0.42 at 373 K. a. Calculate Agºrxn at 373 K. b. Using the value of AHºrxn = 45.38 k) and the AGºrxn calculated in part a, calculate the ASºrxn at 373 K. Consider the reaction: 2NO(g) + C12(8) + 2NOCI(g) Given the following table of thermodynamic data,...
For the reaction 2Fe3+ + 3I− ⇆ 2Fe2+ + I3− (all aq); The initial concentrations of Fe3+ and I− are each 0.300 mol/L. The equilibrium concentration of Fe2+ is 0.16 mol/L. Calculate the equilibrium constant, Kc, for this reaction.
question 1 - Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe3+(aq) + Cu+(aq) Fe2+(aq) + Cu2+(aq) Carry at least 5 significant figures during intermediate calculations to avoid roundoff error when taking the antilogarithm. Equilibrium constant: ..... ? G° for this reaction would be greater or less than zero.? question 2 Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2+(aq) + Hg(l)2Cu+(aq) + Hg2+(aq) Carry at least 5 significant figures during intermediate...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe2+(aq) + 2Fe2+(aq) —>Fe(s) + 2Fe3+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would be - than zero. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe2+(aq) + Cu(s)—— Fe(s) + Cu2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2+(aq) + Hg(l)2Cu+(aq) + Hg2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant... ? G° for this reaction would be greater or less than zero???? question 2 Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Fe3+(aq) + Cu(s)2Fe2+(aq) + Cu2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to...
A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). emf of this cell under standard conditions E∘ = 0.771 V What is the emf for this cell when [Fe3+]= 3.70 M , PH2= 0.95 atm , [Fe2+]= 1.0×10−3 M , and the pH in both compartments is 3.95? Express your answer using two significant figures.
1) Which of the following oxidation-reduction reactions will be spontaneous in the direction written? Select all that apply. Mg2+ (aq) + Be (s) → Mg (s) + Be2+ (aq) Cu2+ (aq) + Zn (s) → Cu (s) + Zn2+ (aq) Hg2+ (aq) + Cu (s) → Hg (l) + Cu2+ (aq) Pb2+ (aq) + Cu (s) → Pb (s) + Cu2+ (aq) Fe2+ (aq) + Pb (s) → Fe (s) + Pb2+ (aq) 2) What is the value (in V)...
True or False t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd2+(aq) + 2Fe2+(aq)Cd(s) + 2Fe3+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: _____G° for this reaction would be(greater/less) than zero