(1) For chemical reactions where all reactants and products are in the gas phase the amount of each gas in the vessel can be expressed either as partial pressures or as concentrations. As such the equilibrium constant for a gas phase reaction can also be expressed in terms of concentrations or pressures. For the general reaction, aA(g)+bB(g)cC(g)+dD(g) Kp=(PA)a(PB)b(PC)c(PD)dandKC=[A][B]b[C]s[D]d It is possible to interconvert between KP and KC using KP=KC(RT)n, where R=0.08314Lbarmol1 K1 and n is the difference in stoichiometric coefficients between gaseous products and gaseous reactants. If we assume that the gaseous reactant and products are "ideal" and the partial pressures of the reactants and products were expressed in bar, then the thermodynamic equilibrium constant, K is the magnitude (or numerical value) of Kp. a) For the reaction 2CH4(g)C2H2(g)+3H2(g),Kc=0.160mol2L2 at 1538C. What is Kp for the reaction at this temperature? b) For the reaction N2(g)+3H2(g)2NH3(g),Kp=3.30103 bar 2 at 328C. What is Kc for the reaction at this temperature