Question

8. Explain Le-Chatelier's principle with the following example
N2 (g) + H2 (g) → 2NH3(e), AH,'= -92.4K]/mol​

Answer 1

Explanation:

sorry but not understand this question properly

Answer 2

Explanation:

LE Chatelier principle: If a system at equilibrium is subjected to a change of pressure, temperature, or the number of moles of a component, there will be a tendency for a net reaction in the direction that reduces the effect of this change.

To see how this works (and you must do so, as this is of such fundamental importance that you simply cannot do any meaningful chemistry without a thorough working understanding of this principle), look again at the hydrogen iodide dissociation reaction

2HI→ H 2 + I 2

(11.2.1)

(11.2.1)2HI→H2+I2

Consider an arbitrary mixture of these three components at equilibrium, and assume that we inject more hydrogen gas into the container. Because the H2 concentration now exceeds its new equilibrium value, the system is no longer in its equilibrium state, so a net reaction now ensues as the system moves to the new state.

The Le Chatelier principle states that the net reaction will be in a direction that tends to reduce the effect of the added H2. This can occur if some of the H2 is consumed by reacting with I2 to form more HI; in other words, a net reaction occurs in the reverse direction. Chemists usually simply say that "the equilibrium shifts to the left"

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