The four gases NH_3, O_2, NO, and H_2O are mixed in a reaction vessel and allowe

Question

The four gases NH_3, O_2, NO, and H_2O are mixed in a reaction vessel and allowed to reach equilibrium in the reaction: 4N H_3(g) + 5O_2(g) 4 NO(g) + 6H_2O(g) Certain changes (see the following table) are then made to this mixture. Considering each change separately, state the effect (increase, i: decrease, d: or no change, nc) that the change has on the equilibrium value of the quantity in the second column (or K_c, if that is specified). The temperature and volume are constant unless otherwise stated.

Explanation / Answer

First, let us state the Le Chatelier principle which deals with changes in an equilibrium:

The statement is as follows:

If any equilibrium is disturbed, that is, change in conditions such as P,T, concentration, partial pressure, etc.., the system will counterbalance such change in order to favour the system's equilbirium.

then

a) adding NO, this is a product, so the shift increases toward the left, thereofre, expect H2O to decrease

b) adding NO, this is a product, so the shift increases toward the left, thereofre, expect O2 to increase

c) removing H2O, a poduct, will shift from left to right, therefore, NO must increase

d) removing O2, a reactant, will shift from right to left , therefore, NH3 must increase

e) Addtion of NH3 has n effect in Kc, since Kc is dependent only of Temperature

f)  removing NO, a poduct, will shift from left to right, therefore, NH3 must decrease

g) adding NH3, a reactant, will shift frm left to rigth, so O2 concentation decreaases

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