Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

1.80 moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen.

Given:

Moles of  Li₃N = 0.60 mol

Firstly write the balanced chemical equation:

6Li(s) + N₂(g) → 2Li₃N(s)

To find the number of moles of lithium:  

2 moles of  Li₃N are produced when 6 moles Li and 1 mol N₂ reacts.

⇒For 0.60 moles Li₃N, 3 x 0.60 = 1.80 moles Li are required.

1.80 moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen.

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We need 1.80 moles of lithium

Explanation:

Step 1: Data given

Moles Li3N = 0.60 moles

Step 2: The balanced equation

6Li(s) + N2(g) → 2Li3N(s)

Step 3: Calculate moles Li

For 2 moles Li3N produced we need 6 moles Li and 1 mol N2

For 0.60 moles Li3N we need 3*0.60 = 1.80 moles Li

We need 1.80 moles of lithium

answer: a chemical reaction

explanation:

im not wrong

sorry i was late, but i don't know what assignment your talking about, i'm in flvs as well, im in earth space science. but u are behind pace bc every class should be in the 3's or 4'