Reference no: EM132647462

Consider the reversible reaction N2↔2N. Equilibrium considerations for this reaction provide insight into how much dissociation of molecular nitrogen (N2) into free nitrogen atoms ( N) occurs at different temperatures and pressures.

a. Express the partial-pressure equilibrium constant Kp(T) for this equilibrium reaction in terms of the te mperature and the Gibbs functions of formation of N2and of N.

b. Develop a set of equations that can be used to solve for the equilibrium mole fractions of N2 and N in a system that contains only N2 molecules and N atoms at a specified temperature and pressure. Your result should be expressed in terms of the partial -pressure equilibrium constant Kp(T) for the given reversible reaction, and the mixture pressure P.

c. Will the dissociation of N2 molecules into free nitrogen atoms increase, decrease, or remain the same with increasing temperature, for a fixed pressure?

d. Will the dissociation of N2 molecules into free nitrogen atoms increase, decrease, or remain the same with increasing pressure, for a fixed temperature?