Calculate the standard Gibbs energy and equilibrium constant at (a) 25 ° C and (b) 50 ° C for the reaction CH4 (g) + 3CI2 (g) - - CHCI3 (i) + 3HCI (g). That the enthalpy of reaction is independent of temperature.

The decomposition of a generic diatomic element in its standard state is represented by the equation....

The decomposition of a generic diatomic element in its standard state is represented by the equation X,(g) – X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.60 kJ · mol- at 2000. K and -63.08 kJ - mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AGf = 4.60 kJ - mol-!. What is K at that temperature? 0.718 K at 2000. K = Incorrect At 3000. K, AGf = -63.08 kJ - mol-. What is K at that temperature? 6.511 K at 3000. K = Incorrect

The Gibbs energy for a reaction Mg(s) + H₂O(g) → MgO(s) + H₂(g) at a particular temperature is AG = -100.0 kJ/mol. At the same time under the sa conditions, A,G° = +341 kJ/mol. Which of the following statements is true? The reaction is at equilibrium and P(H₂O) = P(H₂). The reaction proceeds in the reverse direction to produce more H₂O(g). The reaction proceeds in the forward direction to produce more H₂(g). The reaction is at equilibrium and P(H₂O) > P(H₂). The reaction is at equilibrium and P(H₂O) < P(H2).