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

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SUMMARY

The discussion focuses on calculating the conversion of nitrogen to ammonia at 773 Kelvin using the law of mass action. The equilibrium constant (K) at this temperature is established as 6.9 x 10-5, and the final total pressure is set at 400 bar. The ideal gas behavior is assumed for the calculation, and participants emphasize the importance of correctly applying the law of mass action to derive the fraction of nitrogen converted to ammonia.

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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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