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VashaNatasha [74]
3 years ago
11

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lit

hium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?
Chemistry
2 answers:
Arisa [49]3 years ago
8 0

Answer:

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

miss Akunina [59]3 years ago
7 0

Answer:

12.5 g of Li are needed in order toproduce 0.60 moles of Li₃N

Explanation:

The reaction is:

6Li(s) + N₂(g) → 2Li₃N(s)

If nitrogen is in excess, the lithium is the limiting reactant.

Ratio is 2:6

2 moles of nitride were produced by 6 moles of Li

Then, 0.6 moles of nitride were produced by (0.6 .6)/ 2 = 1.8 moles of Li

Let's convert the moles to mass → 1.8 mol . 6.94 g/ 1mol = 12.5 g of Li

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Explanation:

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Here HA is a protonic acid such as acetic acid, CH_3COOH

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        K_a = \dfrac{[H_3O^{+}] [A^{-}]}{[HA]}

Here, K_a is the dissociation constant of an acid.

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Sedbober [7]

<u>Answer:</u> The energy of one photon of the given light is 3.79\times 10^{-19}J

<u>Explanation:</u>

To calculate the energy of one photon, we use Planck's equation, which is:

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where,

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Putting values in above equation, we get:

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