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.
Learn More
- Learn more about Le Chatelier's Principle brainly.com/question/4356622
- Learn more about Equilibrium brainly.com/question/538664
- Learn more about Equilibrium Constant brainly.com/question/4137132
Keywords: pressure, equilibrium, Le Chatelier's Principle
This statement is false. Everything expands when heated
The reaction between alcohols and acids forms esters.
D Twenty because it has <span>6 of carbon and 14 of hydrogen. </span>
