Consider the dissociation of methane CH4(g) into the elements H2(g) and C (s, graphite). (a) Given that the standard formation enthalpy and entropy of CH4 (g) are fH=74.85kJmol1 and fS=80.67JK1mol1, respectively, at 298K, calculate the value of the equilibrium constant at 298K. (Note that the standard formation enthalpy/entropy of a compound is defined as the change in enthalpy/entropy for the reaction in which 1mol of the compound in its standard state is formed from its elements in their standard states.) (b) Assuming that rH for the above dissociation reaction is independent of temperature, calculate the equilibrium constant at 50C. (c) Calculate the degree of dissociation of methane at 298K and a total pressure of 0.010bar. Here, the standard (reference) pressure (in the expression for equilibrium constant) is chosen to be p=1bar. (d) Without doing any numerical calculations, by using the expression for obtained in (c) and Le Chatelier's principle, explain how the degree of dissociation for this reaction will change as the pressure and temperature are varied