Question

Be sure to answer all parts. When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) ? 2Li3N(s) What is the theoretical yield of Li3N in grams when 12.8 g of Li is heated with 34.9 g of N2? g If the actual yield of Li3N is 6.73 g, what is the percent yield of the reaction? %

          Be sure to answer all parts.

When heated, lithium reacts with nitrogen to form lithium nitride:

6Li(s) + N2(g) ? 2Li3N(s)

What is the theoretical yield of Li3N in grams when 12.8 g of Li is heated with 34.9 g of N2?

g

If the actual yield of Li3N is 6.73 g, what is the percent yield of the reaction?

%

Be sure to answer all parts.

When heated, lithium reacts with nitrogen to form lithium nitride:

6Li(s) + N2(g) ? 2Li3N(s)

What is the theoretical yield of Li3N in grams when 12.8 g of Li is heated with 34.9 g of N2?

g

If the actual yield of Li3N is 6.73 g, what is the percent yield of the reaction?

%

Added by Hannah W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

09/15/2023

Step 1

To do this, we'll use the molar mass of each reactant and the stoichiometry of the balanced equation. The molar mass of Li is 6.94 g/mol, and the molar mass of N2 is 28.02 g/mol. Now, we'll find the moles of each reactant: moles of Li = (12.8 g) / (6.94 g/mol) = Show more…

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When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N2(g) -> 2Li3N(s) What is the theoretical yield of Li3N in grams when 12.8 g of Li is heated with 34.9 g of N2? If the actual yield of Li3N is 6.73 g, what is the percent yield of the reaction?