List three ways in which the yield of ammonia in the reaction above can be improved for a given amount of H2.
To improve the yield of ammonia in a given reaction involving hydrogen gas (H2), there are several approaches you can take. Here are three possible ways:
1. Increasing the pressure: According to Le Chatelier's principle, increasing the pressure of a reaction will shift the equilibrium towards the side with fewer moles of gas. In the synthesis of ammonia (NH3) from hydrogen and nitrogen (N2), there are four moles of gas on the reactant side (N2 + 3H2) and two moles of gas on the product side (2NH3). By increasing the pressure, you can shift the equilibrium towards the product side, thus increasing the yield of ammonia.
2. Removing products continuously: In the reaction to produce ammonia, removing the product (NH3) as it forms will prevent the reaction from reaching equilibrium, pushing it towards the product side. This can be done by employing various separation techniques, such as using a condenser or scrubbing gases to remove ammonia from the reaction mixture. Continuously removing ammonia prompts the reaction to produce more ammonia, thereby increasing the yield.
3. Optimizing temperature: The synthesis of ammonia is an exothermic reaction, meaning it releases heat. According to Le Chatelier's principle, decreasing the temperature will favor the exothermic reaction, thus increasing the yield of ammonia. However, too low of a temperature may slow down the reaction rate, so it is essential to find an optimal temperature that balances the reaction rate and yield.
Overall, these three approaches—increasing the pressure, removing products continuously, and optimizing the temperature—can help improve the yield of ammonia in a given reaction involving hydrogen gas.