Calculating Nitrogen Conversion to Ammonia at 773K Using the Law of Mass Action

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To calculate the fraction of nitrogen converted to ammonia at 773 K using the law of mass action, start by writing the equilibrium expression based on the reaction. The equilibrium constant K, given as 6.9X10-5, relates the concentrations of the reactants and products at equilibrium. Given the initial mixture of one part nitrogen and three parts hydrogen, apply the ideal gas law to find the concentrations at the final pressure of 400 bar. Use the law of mass action to set up the equation and solve for the fraction of nitrogen converted to ammonia. This approach will yield the desired conversion value based on the provided conditions.
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A mixture of one part nitrogen and three parts hydrogen is heated to a temperature of 773 Kelvin. Use the law of mass action to calculate the fraction of nitrogen that is converted (atom to atom) to ammonia if the final total pressure is 400 bar. As alwyas, use 1 bar for the reference pressure, and assume for simplicity that the gases behave ideally. The equilibrium constant K = exp(-dG/RT) at 773 K is 6.9X10-5.

Can someone please give me a hint on how to approach this problem
 
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The best 'approach' is to first right down the "law of mass action'! Exactly what does it say?
 

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