For chemical reactions involving ideal gases, the equilibrium constant K can be expressed either in terms of the concentrations of the gases (in M) or as a function of the partial pressures of the gases (in atmospheres). In the latter case, the equilibrium constant is denoted as Kp to distinguish it from the concentration-based equilibrium constant K. Part A For the reaction 2CH4(g)--><-- C2H2(g) + 3H2(g) K= 0.155 at 1671°C. What is Kp for the reaction at this temperature? Express your answer numerically. Part B For the reaction N2(g) + 3H2(g)--><-- 2NH3(g) = 3.85×10^?3 at 344°C . What is K for the reaction at this temperature? Express your answer numerically.