The decomposition of a generic diatomic element in its standard state is represented by the equation X₂(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.71 kJ - mol-¹ at 2000. K and −55.51 kJ · mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG₁ = 4.71 kJ · mol-¹. What is K at that temperature? K at 2000. K= At 3000. K, AGf = −55.51 kJ - mol-¹. What is K at that temperature? K at 3000. K =

When temperature increases from – 15.0 °C to + 15.0 °C, the thermodynamic equilibrium constant for the reaction increases four times.  Calculate the standard enthalpy for the reaction.

For a certain chemical reaction, the standard Gibbs free energy of reaction is -107. kJ. Calculate the temperature at which the equilibrium constant K = 1.2 × 1020 Round your answer to the nearest degree. T = 0 °C

For a certain reaction, ΔHº = −1.8 x 102 kJ mol−1 and the equilibrium constant at 800. K is 9.1 × 102 . Estimate the temperature at which the equilibrium constant is 1.0 × 106 .

Determine the equilibrium vapor pressure of germanium metal at 326.0 °C. The standard enthalpy of vaporization of germanium is 376.6 kJ/mol and the vapor pressure at 100.0 °C is 1.6E-32 Pa.

he decomposition of a generic diatomic element in its standard state is represented by the equation   12X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.20 kJ·mol−1 at 2000. K and −53.38 kJ·mol−1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, ?, at each temperature. At 2000. K, Δ?f=4.20 kJ·mol−1. What is ? at that temperature? ? at 2000. K=     At 3000. K, Δ?f=−53.38 kJ·mol−1. What is K at that temperature? ? at 3000. K=

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

For a certain chemical reaction, the equilibrium constant  K   =   ×7.7106  at  5.00   °C . Calculate the standard Gibbs free energy of reaction.Round your answer to  2  significant digits.

For a certain chemical reaction, the equilibrium constant K = 2.8 × 104 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. Round your answer to 2 significant digits. AG° = kJ x10 X Ś

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=