Question

Chem help please

Consider the reaction:

?Li(s)+?N2(g)—->?Li3N(s)


Calculate the mass of Lithium nitride formed from 33.6524g of nitrogen gas and 58.7032g lithium

Answer 1

Considering the equation:

Li(s)+N₂(g)—->Li₃N(s)

Balancing this equation will give :

6Li(s)+N₂(g)—->2Li₃N(s)

It can be seen that 6 mol of Li reacts with 1 mol of N₂to produce 2 mol of Li₃N.

Here 33.6524g of nitrogen gas reacts with 58.7032g lithium to produce Li₃N.

Moles of Li = 58.7032 g *
`(1 mol )/(6.94 g) = 8.46 mol Li`

Moles of
`N_(2) = 33.6524 g * (1 mol)/(28 g) = 1.2 mol N_(2)`

Mass of
`Li_(3) N from Li = 8.46 mol Li * (2 mol Li_(3)N)/(6 mol Li)* (34.83 g Li_(3)N)/(1 mol Li_(3)N) = 98.2 g`

Mass of
`Li_(3) N from [tex] N_(2)` = 1.2 mol
`N_(2)` * \frac{2 mol Li_{3}N}{1 mol N2}* \frac{34.83 g Li_{3}N}{1 mol Li_{3}N} = 98.2 g [/tex] = 83.6 g