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Question
Favourable conditions for the NH3 formation by Haber's process are high pressure and low temperature.
Favourable conditions for the NH3 formation by Haber's process are high pressure and low temperature.
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Solution
The correct option is A True
The reaction involved in Haber's process is:
N2+3H2⇌2NH3 This reaction is exothermic (heat released) and has a negative (2−3−1) Δn=−2.
If the temperature is lowered then, the reaction will go in the direction so that the temperature is retained to initial, therefore reaction will go in the forward direction because the reaction is exothermic.
When pressure is increased, then the reaction will shift such that the net pressure decreases, since the forward reaction decreases the pressure, thus forward reaction is favourable.
Hence, by LeChatelier's principle, high pressure and low temperature is favoured.
(If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.)
The reaction involved in Haber's process is:
N2+3H2⇌2NH3 This reaction is exothermic (heat released) and has a negative (2−3−1)
Δn=−2.
If the temperature is lowered then, the reaction will go in the direction so that the temperature is retained to initial, therefore reaction will go in the forward direction because the reaction is exothermic.
When pressure is increased, then the reaction will shift such that the net pressure decreases, since the forward reaction decreases the pressure, thus forward reaction is favourable.
Hence, by LeChatelier's principle, high pressure and low temperature is favoured.
(If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.)
If the temperature is lowered then, the reaction will go in the direction so that the temperature is retained to initial, therefore reaction will go in the forward direction because the reaction is exothermic.
When pressure is increased, then the reaction will shift such that the net pressure decreases, since the forward reaction decreases the pressure, thus forward reaction is favourable.
Hence, by LeChatelier's principle, high pressure and low temperature is favoured.
(If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.)
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