The number of mole of lithium, Li needed for the reaction is 3.2 moles (Option D)
<h3>Balanced equation </h3>
4Li + N₂(g) → 2Li₂N
From the balanced equation above,
2 moles of Li₂N were obtained from 4 moles of Li
<h3>How to determine the mole of lithium needed </h3>
From the balanced equation above,
2 moles of Li₂N were obtained from 4 moles of Li
Therefore,
1.6 moles of Li₂N will be obtained from = (1.6 × 4) / 2 = 3.2 moles of Li
Thus, 3.2 moles of Li are needed for the reaction
Learn more about stoichiometry:
brainly.com/question/14735801
Answer:
1. C
2. E
3. F
4. D
5. A
Explanation:
Here's an oxidation chart to help
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Idk if this is of any help but if you multiply 8 cents times the 250 watts you get 20 then you multiply that but the 24 hrs you are going to be using it for and I got 480
Answer:
3.74L
Explanation:
PV=nRT
V=nRT/P
= 0.25mol*0.0821LatmK^-1*273k/1.50atm
=3.74L
