= 17. Consider the dissociation of methane, {N2(g) + H2(g) = NN3 (8). (1) Using Table 2.8 in Resource Section, calculate the value of the equilibrium constant at 298 K. (2) Assuming that ArxH is independent of temperature, calculate K and Ke at 373 K. (3) Calculate the equilibrium partial pressures of the three gases at 298 K, using the result of 3.(1). Note, 1.0 bar of N, and 3.0 bar of H, are fed to a reactor at an initial condition before the reaction starts. (4) Without doing any numerical calculations, explain how the amount of reactants and products at equilibrium will change as pressure and temperature is increased, respectively. = 17. Consider the dissociation of methane, {N2(g) + H2(g) = NN3 (8). (1) Using Table 2.8 in Resource Section, calculate the value of the equilibrium constant at 298 K. (2) Assuming that ArxH is independent of temperature, calculate K and Ke at 373 K. (3) Calculate the equilibrium partial pressures of the three gases at 298 K, using the result of 3.(1). Note, 1.0 bar of N, and 3.0 bar of H, are fed to a reactor at an initial condition before the reaction starts. (4) Without doing any numerical calculations, explain how the amount of reactants and products at equilibrium will change as pressure and temperature is increased, respectively