How can we increase the total amount of produced Cl 2 during the reaction: 2 ICl (s) ⇄ I 2 (s) + Cl 2 (g)?

By removing the Cl 2 as it is formed

Quiz | Chemical Equilibrium

1

Which of the following statements about the equilibrium constant is correct?

It changes with changes in the temperature

It changes by the addition of a catalyst

It always remains the same at different reaction conditions

It increases if the concentration of one of the reactants or products is increased

According to Le Châtelier's principle, if a dynamic equilibrium is disturbed by changing the conditions, the equilibrium position moves to counteract the change. The quantities whose change may affect an equilibrium are the concentration of a reactant or product, the volume, the pressure and the temperature

Concepts related to this Question

Le Châtelier’s Principle

2

Which of the following statements is correct?

At the equilibrium, sum of [reactant] = sum of [product]

At the equilibrium the forward and reverse reactions still occur

A chemical equilibrium can be attained only starting from a mixture

Chemical equilibrium is a static equilibrium, [reactant] = constant and [product] = constant

Chemical equilibrium is a dynamic equilibrium: the forward and reverse reactions still occur but reactants and products are formed at such rate that their concentration does not change

Concepts related to this Question

Chemical Equilibrium

3

What is the equilibrium constant expression K_C of the reaction: N₂(g) + 3 H₂(g)

⇄

2 NH₃(g)?

$\frac{[N_{2}] [H_{2}]}{[{NH}_{3}]}$

$\frac{[{NH}_{3}]}{[N_{2}] [H_{2}]}$

$\frac{[N_{2}] {[H_{2}]}^{3}}{{[{NH}_{3}]}^{2}}$

$\frac{{[{NH}_{3}]}^{2}}{[N_{2}] {[H_{2}]}^{3}}$

Equilibrium constant K_C: ratio of product concentrations to reactant concentrations at the equilibrium
The concentrations are raised to a power equal to the stoichiometric coefficient

Concepts related to this Question

Equilibrium-Constant Expressions

4

What is the equilibrium constant expression K_C of the reaction: 2 ICl (s) $⇄$ I₂(s) + Cl₂(g)?

[Cl₂]

$\frac{[I_{2}]}{{[ICl]}^{2}}$

$\frac{[{Cl}_{2}] [I_{2}]}{2 [ICl]}$

$\frac{[{Cl}_{2}] [I_{2}]}{{[ICl]}^{2}}$

Equilibrium constant K_C: ratio of product concentrations to reactant concentrations at the equilibrium
Pure solids reactants and products do not appear in the equilibrium-constant expression (= 1 by convention)

Concepts related to this Question

Equilibrium-Constant Expressions

5

How can we increase the total amount of produced Cl₂ during the reaction: 2 ICl (s) $⇄$ I₂(s) + Cl₂(g)?

By adding more ICl

By increasing the pressure

By removing the Cl₂ as it is formed

By decreasing the volume of the container

According to Le Chatelier’ principle, the position of equilibrium will move in such a way as to counteract the change: by removing the Cl₂ as it is formed, the equilibrium will move to the right to produce more Cl₂

Additionally, the right is the side with most moles of gas. The equilibrium will move to the right if the concentration of a reactant decreases OR the volume increases OR the pressure decreases

Concepts related to this Question

Le Châtelier’s Principle

6

What happens when the reaction quotient Q_C is less than the equilibrium constant K?

The reaction will move to the left

The reaction will move to the right

It depends on whether the reaction is endothermic or exothermic

It depends on the reaction conditions

Reaction quotient Q_C: ratio of product concentrations to reactant concentrations at a given time
If Q_C < K, the reaction will move to the right ⇒ net formation of product

Concepts related to this Question

Approach to Equilibrium

Quiz | Chemical Equilibrium

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