Question

One step of the Ostwald process for manufacturing nitric acid involves making nitrogen monoxide by oxidizing ammonia in the presence of a platinum catalyst: 4NH3 (g) + 502 (g)>> 4NO (g) + 6H2O (g). If the percentage yield is 80.3%, how many grams of NO can be produced from 4.00 times 10^3 grams of NH3?
try this;

% yield = (exp. yield)/(theoretical yield) x100%

where exp. yield is the experimental yield (what you actually get)

theoretical yield is calculated from the equation using the mass of NH3 to determine the mass of NO.

hope that helps

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