Lithium and nitrogen react in a combination reaction to produce lithium nitride: . 6li(s)+n2(g)→2li3n(s). in a particular experiment, 5.00-g samples of each reagent are reacted. the theoretical yield of lithium nitride is g.

8.33 g of Lithium Nitride

Explanation:

Well, the answer provided by the user is correct. The problem is that he didn´t explain why he/she did the math using one reactant instead of the other.

When you have more than a reactant with a fixed mass in your experiment, you must consider which is the limiting reactant!

Please, see the picture for deeper details.

All in all, you have 5g of Li and 5g of N2. For 41.4 g of Li you need 28 g of N2, therefore for 5g of Li you´d need 3.38 g of N2 (PLEASE SEE THE PICTURE! Otherwise, it is not easy to see).

Therefore, for 5 g of Li you need 3.38 g of N2 whereas you infact have 5 g! See? There are 1.62 g of N2 that are not taking part in the reaction! So, the N2 is the reactant in excess reagent!!!

All this is correct only if we consider that the reaction has a 100% yield. The exercise does not mention anything about it, so I´ll consider it like this.

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation:

un recipient conține 6,4 moli de gaz. gazul hidrogen reprezintă 25% din totalul kilometrilor din container. în cazul în care presiunea totală este de 1.24 atm ceea ce este