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for the reaction: N2 +O2 ? 2NO. Kc is 0.01 at 2000 degrees celcius. After this...

for the reaction: N2 +O2 ? 2NO. Kc is 0.01 at 2000 degrees celcius. After this system has established equilibrium, 0.015 moles of N2 are added. How does the addition of N2 affect the concentrations of both o2 and NO once equilibrium is established again

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Answer #1

Reaction quotient, Q = [NO]2/([N2]×([O2])

At equilibrium conditions Q= Kc. But when some N2 is added to the system, new Q value becomes smaller than Kc due to increase in the value of denominator in Q expression.

To regain equilibrium when Q will again become equal to Kc, in the expression of Q denominator has to decrease and numerator increase, that is reaction has to shift to right towards formation of more of product, NO. This way amount of O2 will decrease and NO increase at the equilibrium.

Hence concentration of O2 will decrease and that of NO will increase.

Comment in case of any doubt.

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