Given the equation N2+3H22NH3

If 27.7 grams of ammonia is produced by the reaction of 18.4 grams of hydrogen with an excess of nitrogen, what is the percent yield of the reaction?

Question

Given the equation N2+3H2>>2NH3

If 27.7 grams of ammonia is produced by the reaction of 18.4 grams of hydrogen with an excess of nitrogen, what is the percent yield of the reaction?

anonymous · Answer

calculate how much ammonia that 18.4 grams of hydrogen is supposed to produce, then use the percent yield formula to find the percent yield

somy · Answer

$$\sf Percentage~yield  = \frac{ Actual~yield }{ Theoretical~yield }\times 100$$
$\sf Actual~yield$ is the mass of ammonia given in the question as 27.7g 
$\sf Theoretical~yield$ is the mass of ammmonia produced that you gotta calculate using 18.4 g of hydrogen with an excess of nitrogen

somy · Answer

btw you can just play ratio game to get the yielding product since limiting reactant is given :3

dtan5457 · Answer

18 grams of hydrogen, so I just multiply ammonia's mass by 3, right?

dtan5457 · Answer

28/102

roughly 27%

somy · Answer

yeah pretty much