# Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after changing

Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after changing the concentration of the reactant or product. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration C2H4(g)+Cl2>2C2H4Cl2(g)
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after the concentration of C2H4 is increased .
after the concentration of C2H4C12 is increased .

## This Post Has 10 Comments

1. tray71016 says:

The equilibrium will shift in the left direction i.e towards reactant side.

Concentration of nitrogen gas and hydrogen gas will increase whereas concentration of ammonia will decrease.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

If the pressure of the container is increased, according to the Le-Chatelier's principle, the equilibrium will shift in the direction where increase number of moles of gas molecules is taking place.

$N_2 ( g )+ 3 H_2 ( g )\rightleftharpoons 2 NH_3 ( g )$

So, on increasing the pressure the equilibrium will shift in the left direction because number of moles of gases on the left hand side the reaction are more than the number of gaseous moles on right hand side.

Concentration of nitrogen gas and hydrogen gas will increase whereas concentration of ammonia will decrease.

2. mmaglaya1 says:

(B) decrease

(A) decrease

(C) increase

Explanation:

According to Le Chatelier's Principle, the change in any state of the equilibrium say temperature, volume, pressure, or the concentration, the equilibrium will oppose these changes and will shift in such a way that the effect cause must be nullified.

Effect of the change in the pressure :

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 the pressure and thus to nullify this effect or to decrease the pressure, the equilibrium will shift in a direction where there are less number of gaseous molecules.

For the reaction given ,

N₂ (g) + 3H₂ (g) ⇄ 2NH₃ (g)

The number of gaseous molecules in the product (2) is less than the reactant (3 + 1), so the equilibrium will shift in forward direction.

Thus, concentration of N₂ will decrease.

Concentration of H₂ will also decrease.

Concentration of NH₃ will increase.

3. Mynameismath says:

This question appears incomplete

Explanation:

The equation for the formation of iron(III) thiocyanate complex ion is

Fe³⁺ + SCN⁻ ⇄ Fe(SCN)²⁺

Three factors affect the equilibrium of a reaction

temperaturepressure (in gases)concentration

Since the formation of Fe(SCN)²⁺ is an exothermic reaction (delta H is negative); an increase in temperature will favor the backward reaction and more reactants will be produced. When the temperature is however reduced, the forward reaction will be favored and more products will be produced.

When the concentration of the reactants increases, the forward reaction is favored and hence more Fe(SCN)²⁺ is produced. However, when the concentration of Fe(SCN)²⁺ decreases, the backward reaction is favored and more reactants are produced.

4. looloo273 says:

Explanation:

Ag+(aq) + 2NH3 (aq) ⇄ Ag(NH3)2 (aq)

When it comes to question of this sort, the LeChatelier principle should come to mind. The LeChatelier principle states that changes in the temperature, pressure, volume, or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state.

increasing the concentration of Ag+

This would lead to an increase in concentration of reactants, the system would annul or oppose this change by moving towrds the right, favouring the forward reaction.

decreasing the concentration of NH3

This would lead to a decrease in concentration of reactants, the system would annul this change by moving to the left, favourin the backward reaction.

increasing the concentration of Ag(NH3)2

This would lead to an increase in concnetration of products, the system would annul or oppose this change by moving towards the left, favouring the backward reaction.

5. avery2020 says:

Based on Le Chatelier's principle, if the equilibrium of a given system is disturbed by inducing a change in the temperature, pressure or concentration, then the equilibrium will shift in a direction to undo the effect of the change induced.

The given equilibrium is:

2CO(g) + O2(g) ↔ 2CO2(g)

a) If the concentration of CO (reactant) is increased, then the equilibrium will shift to a direction which would lower the concentration of CO i.e. in the forward direction. Therefore,

[CO2] will increase

[CO] and [O2] will decrease

b) If the concentration of CO2 (product) is increased, then the equilibrium will shift to a direction which would lower the concentration of CO2 i.e. in the reverse direction. Therefore,

[CO2] will decrease

[CO] and [O2] will increase.

6. gabriella1232002 says:

After the concentration of H₂ is decreased

H₂+↑Br₂⇒↓2HBr

After the concentration of HBr is increased

↑H₂+↑Br₂⇒2HBr

Explanation:

After the concentration of H₂ is decreased, there will not be enough H₂ to from HBr, so the concentration of HBr will decrease, and the concentration of Br will increase.

After the concentration of HBr is increased, there would be more HBr that will give more H₂ and Br₂.

7. schneidersamant9242 says:

It depends on the nature of the reaction. if the reaction favors high pressure then the reaction will produce more products to reestablish the equilibrium. then if the the chemical reaction favors low pressure then when increasing the pressure the chemical reaction will produce more of the reactants to reestablish equilibrium.

8. crobinson2327 says:

The change in the concentration of the substances in a system to reach equilbrium after changing certain factors like pressure and volume can be explained by the Le Chatelier's Principle. One example would be if you have a system where one of the product is a gas, increasing the pressure would shift the equilibrium towards the formation of the reactants.

9. villatoroo84502 says:

Decrease pressure: Decrease in both reactants, increase in both products

Decrease volume: Increase in both reactants, decrease in both products

Explanation:

10. heyysn3858 says:

1. Br₂ decreased : system moving to the left2. HBr increased : system moving to the leftFurther explanation

In the equilibrium system, according to Le Chatelier, if there is a reaction there will be action

Reaction = - action

If the concentration of one component is enlarged, the system reaction is to reduce the component, and vice versa, if the concentration of one component is reduced, the reaction system is to add to the component

From reaction :

H₂(g) + Br₂(g) ⇔ 2HBr(g)

After the concentration of Br₂ is decreased :

The system will react by increasing the concentration of reagents by moving to the left

After the concentration of HBr is increased.

The system will react by decreasing the concentration of product by moving to the left