1.30 grams of hydrogen gas are reacted with an excess of nitrogen gas to produce 4.21 grams of ammonia. What is the percent yield?

Question

I can calculate percent yield but I am just having a hard time doing dimensional analysis for stoichiometry. Thank you!

2167 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-05-12T05:22:50

19.22 %

In order to get the Percent Yield, first, we have to find its Theoretical Yield.

Solution Map: #grams H->molH->molNH_3->gramsNH_3#

#cancel(1.30g H)*cancel(molH)/cancel(molar mass H)*cancel(molNH_3)/cancel(molH)*(molarmassNH_3)/cancel(molNH_3)#

Therefore,
#cancel(1.30g H)*cancel(mol H)/cancel(1.008g H)*cancel(molNH_3)/cancel(molH)*(17.031g NH_3)/cancel(molNH_3)=color(red)(2.19*10^1g NH_3)#

Now that we have the Theoretical yield, we can solve for the Percent Yield.
#("Actual Yield")/("Theoretical Yield")*100="Percent Yield"#

#color(blue)(4.21gNH_3)/color(red)(2.19*10^1gNH_3)*100=color(pink)19.22%#