The standard state of a substance used to be defined as 1 atm at the specified temperature. By how much does the current definition of standard chemical potential (at 1 bar) differ from its former value at 298.15 K?

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar 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, = 0.250 bar, PH, = 0.100 bar, and PNH, = 0.650 bar? AG = kJ/mol

Σ *00 R The decomposition of a generic diatomic element in its standard state is represented by the equation (3)X – (3)°x{ Assume that the standard molar Gibbs energy at 3000. of formation of X(g) is 5.18 kJ mol- K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. at 2000. K and -62.41 kJ mol- At 2000. K, AG = 5.18 kJ - mol. What is K at that temperature? %3D K at 2000. K = At 3000. K, AG = -62.41 kJ - mol. What is K at that temperature? K at 3000. K = Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Sca 8:10 P (口O回 11/8/20 F7 F10 F12 PrtScr Delete F5 F6 F11 Insert Backspace % 5. B. Alt Ctrl

Calculate the change in the molar Gibbs energy of nitrogen gas when its pressure is increasedisothermally from 1.0 atm to 50.0 atm at 298 K