1. For the following reaction, 1/4 P4(s) + 3/2 H2(g) PH3(g), the corresponding standard Gibbs energy of reaction, rG is +13.4 kJ/mol at 298K. At non-equilibrium condition, determine the reaction Gibbs energy, rG, when the partial pressure of H2 and PH3 (both treated as ideal gases) are 1 bar and 0.6 bar, respectively? What is the spontaneous direction of the reaction in this case?

2. Molecular bromine is 24% dissociated at 1600 K and 1 bar (the total pressure is 1 bar) in the equilibrium Br2(g) 2Br(g). Calculate K at (i) 1600 K and (ii) 2000 K given that rH =+112 kJ/mol over the temperature range. Assume all gases behave ideally, and rH is constant over the studied temperature range. Assume at the initial state, the number of mole of Br2(g) and Br(g) is n mol and 0 mol, respectively.

Please solve both Questions in Detail Thanks.