Equallibrium 2.10 Flashcards
(47 cards)
What is a reversible reaction?
A reaction which goes in both the forward and backward directions.
Reversible reactions can reach a state of equilibrium where the rate of the forward reaction equals the rate of the backward reaction.
What is a dynamic equilibrium?
A dynamic equilibrium is a reversible reaction in which the amount of each reactant/product remains constant and the rate of the forward reaction is equal to the rate of the backward reaction.
What is a homogeneous equilibrium?
A homogeneous equilibrium has everything present in the same phase.
What are common examples of homogeneous equilibrium?
Usual examples include reactions where everything is a gas or everything is present in the same solution.
What is a heterogeneous equilibrium?
A heterogeneous equilibrium has things present in more than one phase.
What are common examples of heterogeneous equilibrium?
Usual examples include reactions involving solids and gases, or solids and liquids.
Example: H2O(g) + C(s) ⇌ H2(g) + CO(g)
What is a homogeneous reaction?
A homogeneous reaction is a reaction in which all the reactants and products are in the same physical state.
What is a heterogeneous reaction?
A heterogeneous reaction is a reaction in which all the reactants and products are not in the same physical state.
What is a dynamic equilibrium?
A dynamic equilibrium can only be achieved in closed systems.
What happens when a closed system is opened?
Conditions can be changed after which the system can be allowed to reach equilibrium again.
What factors can alter the position of equilibrium and product yield?
Changing the concentration of a reactant or product, changing the pressure of a gaseous equilibrium, or changing the temperature.
What happens when the concentration of a reactant is increased?
The position of equilibrium moves to the right, increasing the yield of product.
What happens when the concentration of a product is decreased?
The position of equilibrium moves to the right, increasing the yield of product.
What occurs if the concentration of a reactant is decreased?
The position of equilibrium moves to the left, leading to a decreased yield of product.
What is the effect of increasing product concentration on equilibrium?
The position of equilibrium moves to the left, leading to a decreased yield of product.
How does changing pressure affect equilibrium in gas systems?
An increase in pressure moves the equilibrium to the side with fewer gas molecules, while a decrease in pressure moves it to the side with more gas molecules.
What happens to the equilibrium position when pressure is increased in the Contact process?
The equilibrium shifts to the right, where there are fewer gas molecules (two), increasing the yield of the product.
What happens to the equilibrium position when pressure is decreased in the Contact process?
The equilibrium shifts to the left, where there are more gas molecules (three), decreasing the yield of the product.
How does changing temperature affect equilibrium?
Increasing temperature shifts the equilibrium in the endothermic direction, while decreasing temperature shifts it in the exothermic direction.
What is the effect of increasing temperature in the Haber process?
It decreases product yield as the equilibrium shifts to the left, in the endothermic direction.
What is the effect of decreasing temperature in the Haber process?
It increases product yield as the equilibrium shifts to the right, in the exothermic direction.
What is the role of a catalyst in equilibrium?
A catalyst has no effect on the position of equilibrium; it speeds up both the forward and backward reactions equally.
What is the Haber process equation?
N2(g) + 3H2(g) → 2NH3(g)
What is the enthalpy change (ΔH) for the Haber process?
ΔH = -92 kJ mol-1
