Molecular bromine is 24 per cent dissociated at 1600K and 1.00 bar in the equilibrium Br2(g)2Br(g). Calculate (a) K at 25C, (b) rG, (c) K at 2000C given that rH=+112kJmol1 over the temperature range. In the gas-phase reaction A+BC+2D, it was found that, when 2.00molA,1.00molB, and 3.00molD were mixed and allowed to come to equilibrium at 25C, the resulting mixture contained 0.79molC at a total pressure of 1.00 bar. Calculate (a) the mole fractions of each species at equilibrium, (b) K (c) K, and (d) ,G. The equilibrium constant of a reaction is found to fit the expression In K=A+B/T+C/T3 between 400K and 500K with A=2.04,B=1176K, and C=2.1107K3. Calculate the standard reaction enthalpy and standard reaction entropy at 450K. The equilibrium constant for the reaction N2(g)+O2(g)2NO(g) is 1.69103 at 2300K. A mixture consisting of 5.0g of nitrogen and 2.0g of oxygen in a container of volume 1.0dm3 is heated to 2300K and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium. The dissociation vapour pressure of NH4Cl at 427C is 608kPa but at 459C it has risen to 1115kPa. Calculate (a) the equilibrium constant, (b) the standard reaction Gibbs energy, (c) the standard enthalpy, (d) the standard entropy of dissociation, all at 427C. Assume that the vapour behaves as a perfect gas and that H and S are independent of temperature in the range given