What change would not result in a shift of the equilibrium position to the left?
2 a (g) + b (s) = 3 c (g) + energy ( 2 points)
1) increasing the pressure
2) adding more of gas c to the system
removing some of a from the system
4) cooling the system

Option 1) increasing the pressure will not result in a shift of the equilibrium position to the left. Le Chatelier's Principle states that when the pressure is increased the equilibrium will shift to the direction where fewer moles of gas is produced. Since there are equal moles of gas on the left and right side of the equation, the increased pressure will not affect the equilibrium.

Further Explanation:

Option 2) adding more of gas C to the system SHIFTS  THE EQUILIBRIUM POSITION TO THE LEFT because increasing the amount of gas on the right side can be relieved by using up the added C to form A and B.

Option 3) removing some of A from the system SHIFTS THE EQUILIBRIUM POSITION TO THE LEFT because the system will restore the lost reactant by using up C to form more of A.

Option 4) cooling the system SHIFTS THE EQUILIBRIUM POSITION TO THE LEFT because the forward reaction is exothermic. Therefore, removing heat from the system will drive the backward reaction to occur.

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Keywords: pressure, equilibrium, Le Chatelier's Principle

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explanation: