It will shift toward the reactant side as there are a greater number of moles of gas on the reactant side.
Pressure changes only affects only equilibrium involving a gas or gases. An increase in pressure shifts the equilibrium in the direction of the reaction with lower volume.
N₂ + 3H₂ ⇆ 2NH₃
An increase in pressure will shift the equilibrium towards the product side.
If the pressure is decreased, equilibrium will shifts towards the side of the reactants. This is because the volume of the reactants are higher than that of the product.
Based on Le Chatelier's principle, an increase in temperature will shift the equilibrium position towards the products in an endothermic reaction.
An endothermic reaction is a reaction that absorbs heat from the surroundings.
A rise in temperature shifts equilibrium position to the direction that absorbs the heat and vice versa.
In an endothermic reaction, the forward reaction absorbs the heat and therefore equilibrium shifts towards the side of product.
Decreasing the pressure A) Shift to the left
Adding hydrogen gas B) Shift to the right
Adding a catalyst C) No effect
N₂ + 3H₂ ⇆ 2NH₃
Pressure : Decreasing the pressure will shift the equilibrium position to the left. In reactions involving gases, increase in pressure favors the side with a lesser volume. An increase in pressure will favor the formation of ammonia as a product.
A decrease in pressure shifts the equilibrium to the left towards the side of high volume.
Concentration: addition of hydrogen gas will increase the concentration of the gas. An increase in concentration favors the side that uses up the specie and lowers it concentration.
If the concentration of hydrogen gas is increased the equilibrium will shift to the right to annul the concentration of reactants that has increased.
Catalyst: Catalysts have no effect on the position of chemical equilibrium. It only affects the rate at which equilibrium can be reached.
Adding more of gas C to the system
The change that would shift the equilibrium system to the left is by adding more of gas C to the system.
This will increase the concentration of gas C, in order to annul this, the equilibrium will shift to the left.Heating the system will shift the equilibrium to the rightIncreasing volume only affects purely gaseous reactions. Removing some of gas C from the system shifts the equilibrium to the right.
Heating the system
This is an exothermic reaction because enthalpy change is negative. A rise in temperature shifts equilibrium position to the direction that absorbs heat.
In an exothermic reaction, heat is given off in the forward process. The reverse process is endothermic and heat is absorbed.
Therefore, heating the system will shift the equilibrium to the left and heat is absorbed.
This reaction is exothermic because the system shifted to the left on heating.
It is right to conclude that this reaction is exothermic because the system shifted to the left on heating .
Since the reaction turned dark brown on heating, it shows that more of the reactant Nitrogen dioxide gas was produced.
We can see that the reaction is exothermic in the forward process. An increase in temperature shifts equilibrium position backward to the side that absorbs the heat. This allows for the production of more nitrogen dioxide.
Shift it toward the reactants
A decrease in the concentration of the reactants shift the reaction towards the sides of the reactants.
An increase in concentration of a specie favors the direction that uses up that specie and lowers its concentration.
If the concentration of a specie on the reactant side is increased, equilibrium shifts to the right where more products are formed.
if we decrease the concentration of reactants, the products will be more concentrated and the equilibrium will shift to the left i.e the reactant side.
Question 1: 1) Increasing the pressure C) Shift to the right
2) Removing hydrogen gas A) Shift to the left
3) Adding a catalyst B) No effect
Question 2: This reaction is exothermic because the system shifted to the right on cooling.
Question 3: Shift it toward the reactants.
Question 4: Adding more of gas C to the system.
Question 5: It will shift toward the reactant side because the reactant side has one more mole of gas than the product side.
Question 6: True.
Question 7: there is no suitable choice is provided.
We can shift the equilibrium toward the right via:
Increasing N2O3 concentration,
decreasing NO and/or NO2 concentration,
decreasing the pressure,
lowering the T (cooling the system).
Question 1: Match the action to the effect on the equilibrium position for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g).
Removing ammoniaA) No effect
Removing hydrogen gasB) Shift to the left
Adding a catalystC) Shift to the rightLe Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.
1) Increasing the pressure:When there is an increase in pressure, the equilibrium will shift towards the side with fewer moles of gas of the reaction. And when there is a decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.The reactants side (left) has 4.0 moles of gases and the products side (right) has 2.0 moles of gases.So, increasing the pressure will shift the reaction to the side with lower moles of gas (right side).
so, the right match is: C) Shift to the right.
2) Removing hydrogen gas:Removing hydrogen gas will decrease the concentration of the products side, so the reaction will be shifted to the lift side to suppress the decrease in the concentration of hydrogen gas by removing.
so, the right match is: A) Shift to the left.
3) Adding a catalyst:Catalyst increases the rate of the reaction without affecting the equilibrium position.Catalyst increases the rate via lowering the activation energy of the reaction.This can occur via passing the reaction in alternative pathway (changing the mechanism).The activation energy is the difference in potential energies between the reactants and transition state (for the forward reaction) and it is the difference in potential energies between the products and transition state (for the reverse reaction).in the presence of a catalyst, the activation energy is lowered by lowering the energy of the transition state, which is the rate-determining step, catalysts reduce the required energy of activation to allow a reaction to proceed and, in the case of a reversible reaction, reach equilibrium more rapidly.with adding a catalyst, both the forward and reverse reaction rates will speed up equally, which allowing the system to reach equilibrium faster.
so, the right match is: B) No effect.
Question 2: Nitrogen dioxide gas is dark brown in color and remains in equilibrium with dinitrogen tetroxide gas, which is colorless.
2NO2(g) ⇌ N2O4(g)
When the light brown color equilibrium mixture was moved from room temperature to a lower temperature, the mixture turned lighter brown in color. Which of the following conclusions about this equilibrium mixture is true?Moving from room temperature to a lower temperature, means that the T is decreased.The mixture turned lighter brown in color, means that the reaction is shifted towards the products side.Moving towards the product side, means that we decreased the concentration of the product side, which ,means that the heat is evolved from the reaction and the reaction is exothermic.
So, the right choice is: This reaction is exothermic because the system shifted to the right on cooling.
Question 3: According to Le Châtelier's principle, how will a decrease in concentration of a reactant affect the equilibrium system?A decrease in the reactants concentration will disturb the equilibrium position of the system. To attain the equilibrium again, the system will be shifted to the lift (reactants side) to increases the concentration of the reactants and attain the equilibrium again.
So, the right choice is: Shift it toward the reactants.
Note: The answer of Q 4, 5, 6 & 7 and all answers are in the attached word file.