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3 years ago

In the important industrial process for producing ammonia (the Haber Process), the overall reaction is:

Chemistry

1 answer:

Kisachek [45]3 years ago

5 0

Answer:

Explanation:

Here we have to use stoichiometry.

First of all, we have to calculate the mass of 100% of yield:

1.7 g ------- 98%

X -------- 100%

X = 1.73 g (approximately)

Second, we have to calculate the mass of N2 that is necessary to react to produce the mass of 1.73g of NH3. To do that, we have to use the Molar mass of N2 and NH3 and don't forget the stoichiometric relationship between them.

Molar Mass N2 : 14x2 = 28 g/mol

Molar Mass NH3: 14 + 3 = 17 g/mol

28g (N2) ------- 17x2 (NH3)

X ------------ 1.73 g

X = 1.42 g (approximately)

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4 years ago

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hammer [34]

Answer: alkaline earth metals (group-IIA)

Explanation:

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$[Be]:4:1s^22s^2$

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1 year ago

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SpyIntel [72]

Answer:

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Explanation:

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