Question

In 1909 Fritz Haber discovered the workable conditions under which nitrogen, N2(g), and hydrogen, H2(g), would combine using to produce ammonia. The conditions included medium temperature (~500oC), very high pressure (~351kPa), and an iron catalyst. The reaction is represented by the equation: N2(g) + 3H2(g) → 2NH3(g) How many grams of nitrogen are needed to produce 100 grams of ammonia gas?

Answer 1

Answer: 51.8

Step-by-step explanation:

Answer 2

Answer : 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

Solution : Given,

Mass of
`NH_3` = 100 g

Molar mass of
`NH_3` = 27 g/mole

Molar mass of
`N_2` = 28 g/mole

First we have to calculate moles of
`NH_3`.

`\text{ Moles of }NH_3=\frac{\text{ Mass of }NH_3}{\text{ Molar mass of }NH_3}= (100g)/(27g/mole)=3.7moles`

The given balanced chemical reaction is,

`N_2(g)+3H_2(g)\rightarrow 2NH_3(g)`

From the given reaction, we conclude that

2 moles of
`NH_3` produced from 1 mole of
`N_2`

3.7 moles of
`NH_3` produced from
`(1mole)/(2mole)* 3.7mole=1.85moles` of
`N_2`

Now we have to calculate the mass of
`N_2`.

Mass of
`N_2` = Moles of
`N_2` × Molar mass of
`N_2`

Mass of
`N_2` = 1.85 mole × 28 g/mole = 51.8 g

Therefore, 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.