For a certain chemical reaction, the standard Gibbs free energy of reaction is 83.7 kJ. Calculate the temperature at which the equilibrium constant K = 1.9x 10-16 Round your answer to the nearest degree.

For a certain chemical reaction, the standard Gibbs free energy of reaction at  15.0   °C  is  147.   kJ . Calculate the equilibrium constant  K  for this reaction.Round your answer to  2  significant digits.

For a certain chemical reaction, the standard Gibbs free energy of reaction at 30.0°C is 73.3 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits.

Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(s) +20₂(g) → M₂O4(s) For this reaction, AH = -4.961 kJ/mol and AS ixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGixn= What is the equilibrium constant of this reaction at 298 K? Kp = What is the equilibrium pressure of O₂(g) over M(s) at 298 K? MacBook Pro tyne URI + kJ/mol O

The equilibrium constant for a system at chemical equilibrium at 318 oC is 3.4 x 10-3.  Calculate the Gibbs free-energy change, deltaGo, for the system at 318 oC.Enter your answer here: kJ/mol

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N, (g) + 3 H, (g) = 2 NH,(g) the standard change in Gibbs free energy is AG° = –72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.500 atm, PH, = 0.500 atm, and PNH, = 0.600 atm? AG = kJ/mol

Enter your answer in the provided box. Kf for the complex ion Ag(NH3)2+ is 1.5 × 107 at 25 ° C. Using this information, calculate the value of Δ G o   f for Ag(NH3)2+(aq).

Determine the molar ΔH°solution for a soluble ionic compound when the dissolution of 0.171 moles of that compound leads to a 12.9 °C temperature increase in a constant pressure calorimeter. The heat capacity of the calorimeter is 1.120 kJ/℃.

For a certain chemical reaction, the standard Gibbs free energy of reaction is -133. kJ. Calculate the temperature at which the equilibrium constant K = 8.2 x 10- 22 Round your answer to the nearest degree. T= \| °C

For a certain chemical reaction, the standard Gibbs free energy of reaction is - 149. kJ. Calculate the temperature at which the equilibrium constant K = 1.3 × 1026. Round your answer to the nearest degree. T=