For the reaction: 2 NO_(g) + Cl2_(g) = 2 NOCI_(g) (The = symbol represents equil

Question

For the reaction: 2 NO_(g) + Cl2_(g) = 2 NOCI_(g) (The = symbol represents equilibrium arrows.) How does the concentration of NO change when NOCl is removed from the equilibrium mixture? The reaction goes to the left (leftarrow), the concentration of NO decreases. The reaction goes to the left (leftarrow), the concentration of NO increases. The reaction goes to the right (rightarrow), the concentration of NO increases. The reaction goes to the right (rightarrow) the concentration of NO decreases.

Explanation / Answer

Ans. Le Chatelier’s principle “if a dynamic equilibrium is disturbed by changing the conditions (Concentration, Volume, Pressure, temperature, etc.), the position of equilibrium shifts to counteract the change to reestablish an equilibrium”

            Balanced reaction: 2 NO2(g) + Cl2(g) -----------> 2 NOCl(g)

When NOCl is removed from the system, the net reaction proceeds in right (forward) direction to produce more NOCl- therefore counteract to compensate the loss of NOCl by producing more NOCl. The net forward reaction stops after new equilibrium is established.

So, when the reaction proceeds in forward direction more NO is converted into products (NOCl)- therefore [NO] decreases.

Option A, and B are incorrect because the reaction can’t go in left (backward) direction. Option C is incorrect because [NO] must decrease when the reaction proceeds in forward direction.

Correct option- D.

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