Ammonia Synthesis Lab Report

To go in more depth, 98.2% is a high yield, despite the inaccuracies due to time constraints, and the inability to the recrystallize the benzoic acid. As mentioned earlier, product might have been lost during the many filtration procedures in the experiment, as not all of the product was poured out from the flask, onto the filter. Since, recrystallization could not be done, the benzoic acid was immediately transferred onto the watch glass, and it is when transferring some product could have been left on the filter. Overall, pouring product into the filter, and trying to get every particle of product from the flask for each filtration procedure in the experiment, is rather difficult, and is impossible to get every bit of product. Another key possibility, though it fortunately did not occur in the experiment, a green, or purple result

Given ammonia is obtained in 90% yield, the amount of hydrogen necessary to produce 100Mg of ammonia can be calculated by using Equation #1, except reformulated to solving for the maximum possible ammonia mass, hence, maximum possible ammonia mass= (100Mg of ammonia ×100%)/(90%), which equals to 111Mg. The mass must be converted into moles, thus, (111 Mg of ammonia)×((1,000,000 g)/(1 Mg))×((1 mole)/(17.031 g)), which is 6,524,100 moles of ammonia. The chemical structure of ammonia is NH3 meaning there are 3 hydrogen atoms per ammonia molecule. Thus, the calculation of the number of moles of hydrogen atoms can be found using, (6,524,100 moles of ammonia)×((3 moles of hydrogen)/(1 mole of ammonia)), equaling to 19,572,000 moles of hydrogen atoms. Lastly, convert from moles to tons of hydrogen by using the molar mass of hydrogen, and the fact that 1 gram is equivalent to 1.10231×〖10〗^(-6) tons. Therefore, the formula is, (19,572,000 moles of hydrogen atoms)×((1 grams)/(1.00794 moles of hydrogen atoms))×((1.10231*〖10〗^(-6))/(1 grams)), which leaves the final result of 21.404 tons of hydrogen is necessary to produce 100Mg of