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NEETChemistryChemical Equilibrium

For the equilibrium reaction of the formation of nitric oxide: N ₂( g ) + O ₂( g ) 2 NO ( g ), H = +180.7 kJ Which of the following conditions will favour the maximum yield of NO ?

Options

  1. AHigh temperature, high pressure and high concentration of N ₂
  2. BHigh temperature, high concentration of O ₂ , and pressure has no effect
  3. CLow temperature, high pressure and high concentration of N ₂
  4. DLow temperature, low pressure and low concentration of O ₂

Correct answer

B. High temperature, high concentration of O ₂ , and pressure has no effect

Step-by-step solution

According to Le Chatelier's principle: 1. The given reaction is endothermic ( H > 0 ). Endothermic reactions are favoured in the forward direction at high temperatures. 2. The change in the number of gaseous moles is n _g = 2 - (1 + 1) = 0 . Since there is no change in the number of moles of gases, a change in pressure has no effect on the equilibrium position. 3. Increasing the concentration of reactants ( N ₂ or O ₂ ) shifts the equilibrium in the forward direction to consume the added reactants. Therefore, high

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