Question

The Haber process is a reversible reaction.
N2(g) + 3H2(g) 2NH3(g)
The reaction has a 30% yield of ammonia.
Which volume of ammonia gas, NH3, measured at room temperature and pressure, is obtained
by reacting 0.75 moles of hydrogen with excess nitrogen?
(A) 3600 cm3 (B) 5400 cm3 (C) 12 000cm3 (D) 18 000cm3
Above are the options given!!
An answer would be much appreciated!!

Answer 1

Answer:

N

2

+3H

2

⇌2NH

3

+QKcal

(i) since process of making ammonia is exothermic process low temperature is favourable

(ii) No. of mole of gase is reactant side is more than product side so high pressure is favourable in production of Ammonia

According to above two condition low temp and high pressure is favourable

⇒ Option C is correct.

Answer 2

Answer:

N2 + 3H2⇌2NH3+QKcal

Low temperatures are desirable since the production of ammonia is an exothermic process. High pressure is helpful for creating ammonia because there are more gas molecules on the reactant side of a reaction than on the product side. Ideally, it should be $12 000cm3$

Explanation:

The Haber Process is used to create ammonia from nitrogen and hydrogen and then goes on to describe the rationale for the process's parameters. The procedure creates ammonia by coupling airborne nitrogen with hydrogen primarily generated from natural gas (methane).

Equilibrium is where several crucial chemical reactions take place. One such is the Haber process, which produces ammonia—a major fertilizer used today to boost agricultural yield—by combining nitrogen and hydrogen gas.

The production of ammonia may be altered by altering the reaction's pressure or temperature since the Haber process is a reversible reaction. The yield of ammonia rises as the reaction pressure increases. It is noticed to the reversible reaction of the Haber process.

To learn more about the Harber process visit:

https://brainly.in/question/1561090

To learn more about the reversible reaction, visit:

https://brainly.com/question/22406030

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