For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction N₂(g) + 3H₂(g)2NH, (g) the standard change in Gibbs free energy is AG = -69.0 kJ/mol. What is AG for this reaction at 298 K when the partial = 0.650 bar? pressures are P, = 0.400 bar, PH, = 0.200 bar, and PNH, AG = x10 TOOLS kJ/mol

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Part A The value of K, for nitrous acid (HNO,) at 25 °Cis 4.5 x 10 4 Part B Part C What is the value of AG at equilibrium? Express your answer using one significant figure. AG = 0 kJ Submit Previous Answers v Correct By definition, the Gibbs free energy of a reaction is zero when it is at equilibrium. Forward and reverse reactions continue to occur dynamically, but there is Part D What is the value of AG when [H'] = 5.1 x 10 2 M. [NO,] = 6.2 x 10 4M and (HNO2] = 0.21 M? Express your answer using three significant figure. ? AG = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

For the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 22.7 at 25oC and 36.5 at 50oC. What is the value of the standard Gibbs free energy change (in kJ) of this reaction at 75oC?