Consider the reaction:
A (aq) ⇌ B (aq)
at 297 K under standard conditions. If ΔGo is -5.69 kJ
at this temperature, how much must the concentration of "reactant
A" change for the non-standard Gibb's Free energy to be -1.55
kJ?
Consider the reaction: A (aq) ⇌ B (aq) at 297 K under standard conditions. If ΔGo...
For the reaction Fe(s) + 2HCI(aq)FeCl2(s) + H2(g) ΔΗο--7.4 kJ and ΔS°-107.9 J/K The standard free energy change for the reaction of 2.11 moles of Fe(s) at 278 K, 1 atm would be -37.4kJ This reaction is (reactant, product) -78.9 favored under standard conditions at 278 K Assume that Δ Ho and Δ are independent of temperature. For the reaction N2(g) + O2(g)2 NO(g) Δσ 172.7 kJ and ΔS°-24.9 J/K at 318 K and 1 atm. This reaction is (reactant,...
Under standard conditions, the ΔGo of the reactants for a given redox reaction is measured to be 209.8 kJ and the ΔGo of products is measured to be 168.1 kJ. If 2 moles of electrons are required in the balanced redox reaction, calculate the standard cell potential, Eocell, for the reaction described here at 25 oC.
For the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) H° = -7.4 kJ and S° = 107.9 J/K The standard free energy change for the reaction of 1.54 moles of Fe(s) at 315 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 315 K. Assume that H° and S° are independent of temperature.
PLEASE ANSWER ALL 5 QUESTIONS (2 on standard entropy of reaction, 3 on Delta G) AND SHOW ALL WORK! *If you do not anticipate to answer all posted questions in given post, please leave unaswered for someone else to help me with them ALL* Consider the reaction: CaCo3(s) Cao(s)+Co2g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.20 moles of CaCOs(s) react at J/K AS system Submit Answer Consider the reaction: 2C2Ho(g)+702)4Co2(g)+ 6H20) Using...
Consider the following phosphate transfer reaction that is exergonic under standard conditions: A~P + B → B~P + A The standard free energy for A~P → A + Pi is -25.6 kj/mol What can be predicted for the standard free energy of: B + Pi --> B~P ? a. -25.6 kj/mol b. -12.0 kj/mol c. +12.0 kj/mol d. +25.6 kj/mol e. None of the above
Consider the reaction Ca(OH)2(aq) + 2HCl(aq)CaCl2(s) + 2H2O(l) for which H° = -30.20 kJ and S° = 205.9 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.934 moles of Ca(OH)2(aq) react under standard conditions at 298.15 K. Suniverse = ----------J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is...
NH4Cl(aq) NH3(g) + HCl(aq) G° = 62.3 kJ and H° = 86.4 kJ at 305 K and 1 atm. This reaction is (reactant, product)----- favored under standard conditions at 305 K. The entropy change for the reaction of 2.30 moles of NH4Cl(aq) at this temperature would be ------- J/K.
For an equilibrium reaction, ΔG = 0 kJ at 432.6 K. If the standard change in Gibb's free energy of this reaction is 0.344 kJ, what is the equilibrium constant?
For the reaction: Cu+ (aq) + 2 NH3 (aq) --> [Cu(NH3)2]+ (aq) The K value is 6.3x1010. What is the non-standard Gibb's free energy of the reaction (Grxn) when the concentrations are adjusted to [Cu+] = 0.100 M, [NH3] = 0.100M, and the [Cu(NH3)2]+ = 1.0 x 10-3 M.
For the reaction 2 A(aq) ⇋ B(aq) + C(aq), the value of ΔGo is 3.92 kJ at 25.0oC. If the initial concentrations of A(aq), B(aq), and C(aq) are respectively 0.484 M, 0.328 M, and 0.254 M, what will be the concentration of A(aq) when we reach equilibrium at 25.0oC?