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Problem: What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation?Li + N2 ⟶ Li3N

🤓 Based on our data, we think this question is relevant for Professor Ho's class at QC CUNY .

FREE Expert Solution
FREE Expert Solution

Recall that the limiting reactant will produce the LEAST BUT CORRECT amount of products

Balanced equation will appear as:

6 Li + N2 ⟶ 2 Li3N

MM of Li and N2 is 6.94 g/mol and 28.02 g/mol

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Problem Details

What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation?

Li + N2 ⟶ Li3N

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Based on our data, we think this problem is relevant for Professor Ho's class at QC CUNY .

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.