Consider the reversible reaction between nitrogen and
hydrogen gases shown below.
N2(g) + 3H2(g) + 2NH3(9)
In a certain experiment nitrogen and hydrogen gases are
introduced into a reaction vessel Which statement is true?
a
The rate of the reverse reaction increases as time
goes by
b initially, only the forward reaction takes place
The rate of the forward reaction decronses asume
does by

Ammonia is manufactured from nitrogen and hydrogen by the Haber process: N2(g) + 3H2(g) 2 NH3(g) The forward reaction is exothermic. The conditions used in the Haber process are: 200 atmospheres pressure • 450 °C • iron catalyst.

Explanation:

Answer Link

adefioyelaoye adefioyelaoye · Answer 2 · 2022-05-12T13:59:38+02:00

Initially, only the forward reaction taking place in the vessel is a true statement and is denoted as option B.

What is Haber process?

This is defined as the industrial method which is used in the production of ammonia and involves nitrogen fixation with Hydrogen.

During this process, the forward reaction taking place in the vessel before the backward reaction which is why it has a 30 percent ammonia yield.

Read more about Haber process here https://brainly.com/question/21867752

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