Problem: How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.6 Li(s) + N2(g) → 2 Li3N(s)a. 18.3 g Li3Nb. 58.3 g Li3Nc. 61.0 g Li3Nd. 15.1 g Li3Ne. 20.3 g Li3N

FREE Expert Solution

We have to determine how many grams of Li3N can be produced from 1.75 mol of Li.

We will begin solving this problem by analyzing what information we have to solve this problem:


https://lh3.googleusercontent.com/mElibg3hZEJJoTAJ75A-1nrt7O5jaEZT-eoOjP7_SuoEVG8Q77zrQow1Xf3iQ6hsGvB4RxFe6Dcob96AX9I3OAOBngimYA7TCNKm_QYvgMYeZyLNd06R_RQSmDSgygOzfAjdPNMD


We will solve this problem through these steps:

  1. Find the molar mass of Li3N.
  2. Make a mole-to-mole comparison between Li and Li3N to find the number of moles of Li3N.
  3. Find the mass of Li3N using its number of moles and molar mass.


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Problem Details

How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.

6 Li(s) + N2(g) → 2 Li3N(s)

a. 18.3 g Li3N

b. 58.3 g Li3N

c. 61.0 g Li3N

d. 15.1 g Li3N

e. 20.3 g Li3N

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Abraham's class at Frederick Community College.