Respuesta :
Answer:
D
Explanation:
The direction of the reaction by changing the concentration can be determined by Le Chatelier's principle,
It states that ,
When a reaction is at equilibrium , Changing the concentration , pressure, temperature disturbs the equilibrium , and the reaction again tries to attain equilibrium by counteracting the change.
According to Le Chatelier's principle,
If the pressure is increased , the equilibrium of the reaction is disturbed , so, the reaction will move in order to decrease the pressure.
The molecules of gas are responsible for pressure , So, To decrease the pressure reaction will go towards the side with less number of gaseous molecules.
Effect of change in volume -
Pressure and volume of the system are inversely proportional to each other. So if the volume of the system is decreased, the pressure of the system will increase and hence, equilibrium of the system will be disturbed. In order to attain equilibrium again, system will move towards the side having less no. of gaseous molecules to decrease pressure.
A)
Gaseous molecules on right side = 0
Gaseous molecules on left side = 1
Gaseous molecules on right side < Gaseous molecules on left side, the equilibrium will shift right.
B)
Gaseous molecules on right side = 2
Gaseous molecules on left side = 2
Gaseous molecules on right side = Gaseous molecules on left side, the equilibrium will not be attained.
C)
Gaseous molecules on right side = 2
Gaseous molecules on left side = 2
Gaseous molecules on right side = Gaseous molecules on left side, the equilibrium will not be attained.
D)
Gaseous molecules on right side = 3
Gaseous molecules on left side = 2
Gaseous molecules on right side > Gaseous molecules on left side, the equilibrium will shift left.
E)
Gaseous molecules on right side = 2
Gaseous molecules on left side = 4
Gaseous molecules on right side < Gaseous molecules on left side, the equilibrium will shift right.
The principle of Le gave the shift in the equilibrium of the reaction. The equilibrium of the reaction [tex]\rm 2 SO_{3} \leftrightarrow (g) 2 SO_{2} (g) + O_{2} (g)[/tex] will shift to the left when the volume is decreased.
What is equilibrium shift?
Equilibrium shift is the change of the reaction direction when the volume of the reactant or the product is altered or by the change of concentration.
The volume and the pressure of the reaction are inversely proportional to the law and the decrease in the volume will increase the pressure of the reaction.
In the first reaction, the molecules of the gas on the left side is more compared to the right side of the reaction and hence the equilibrium will shift towards the right.
In the second reaction, of the formation of the hydrochloric acid, the gas molecules on the left and the right side of the equation are the same and the equilibrium will not be attained.
Similarly in the third reaction, the number of the gaseous molecules is the same on both sides of the reaction and hence the equilibrium will not be attained.
In the fourth reaction, the gaseous molecule is more on the right side compared to the left of the reaction and hence the reaction will shift towards the left side.
In the fifth reaction, gaseous molecules are more on the left side compared to the right side of the reaction and hence the equilibrium will shift towards the right side of the reaction.
Therefore, option D. [tex]\rm 2 SO_{3} \leftrightarrow (g) 2 SO_{2} (g) + O_{2} (g)[/tex] equilibrium will shift to the left due to a decrease in the volume.
Learn more about equilibrium shift here:
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