Material Energy and Balance The production of Ammonia takes place in an isotherm

Question

Material Energy and Balance The production of Ammonia takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 20.0 volume percent N_2 and the balance is H_2 at an initial pressure of 380 kPa (absolute) Assuming ideal gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of N_2 is 80% Suppose the pressure in the reactor eventually of N_2 is 80% Calculate the reaction equilibrium constant at the prevailing temperature kP[(atm)^-2]

Explanation / Answer

a) the composition of mixture will be similar to volume composition

so mole fraction of N2 = 20 / 100 = 20%

Let initally 100moles are present then out of these the moles of N2 = 20

The moles of N2 converted = 80% of 20 moles = 16 moles

as per stoichiometry 16 moles of N2 will react with 48 moles to give 32 moles of NH3

So total moles present = 4 moles of N2 + 32 moles of H2 + 32 moles of NH3 = 68 moles

Mole fractions

N2 = 4 X 100/ 68 = 0.058 X 100 = 5.9%

H2 = 32 / 68 = 47.05%

NH3 = 32 / 68 = 47.05%

as volume and temperature are constant

So P1 / n1 = P2 / n2

380 kPa / 100 = P2 / 68

P2 = 258.4 K Pa

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