2(g)+3H2(g)-2NH3(g) The reaction is exothermic. Suppose a mixture of N2, H2 and

Question

2(g)+3H2(g)-2NH3(g) The reaction is exothermic. Suppose a mixture of N2, H2 and NH; has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation shift in equilibrium O to the right O to the left O (none) change in composition The temperature is The pressure of N2 will lowered O to the left sure of NH will 2 O (none) 0 Type here to search

Explanation / Answer

The equillibrium reaction is...

N2(g) + 3H2(g) 2NH3(g)

(i) According to Le-Chatelier's principle, if the product is removed then equilibrium shifts to the right to form more product. In that case the rectanats would decreases and their pressures decreases.

(ii) If H2 is added then reaction equilibrium would again shift to the right and the product is formed. Pressure of N2 decreases and pressure of NH3 is increased.

(iii) An increase in volume favors more moles. For the data we have more moles on left side(reactant side). reactant side has 4 moles where as product side has only 2 moles. So, an increase in volume would shift the equilibrium to the left and so the pressure of NH3 will decrease.

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