Question

in haber's process 7 g of Nitrogen is take how manu grams of H2 should be taken such that ratio of N2 and h2 gas remains same throughout the reaction ​

Answer 1

Answer:

N2 + 3H2 → 2NH3

1mol N2 will produce 2mol NH3

Molar mass N2 = 28g/mol

Molar mass NH3 = 17g/mol

28g N2 will produce 2*17 = 34g NH3

7g N2 will produce 7g/28g * 34gNH3

Mass of NH3 produced = 8.5 g NH3

If actual production = 1.8g NH3 , % yield = 1.8g NH3/8.5g NH3 * 100 =21.176%

Answer: Yield = 21% 2 significant digits.

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Answer 2

Explanation:

The Haber Process is used in the manufacturing of ammonia from nitrogen and hydrogen, and then goes on to explain the reasons for the conditions used in the process. The process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.

N2(g)+3H2(g)↽−−⇀2NH3(g)(1)

with ΔH=−92.4kJ/mol .