Question

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?

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

Answer 1

19.22 %

Explanation:

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%`