Basics of Reactions
A reaction that can proceed in both the forward and backward directions to a considerable extent.
A reaction that can proceed in both the forward and backward directions to a considerable extent.
This is the only factor that can actually change the numerical value of the equilibrium constant (K).
Temperature
If you add more reactants to a system at equilibrium, the system will shift in this direction.
Right (Forward)
Conditions in the Haber-Bosch that may not always give the greatest yield of product, but are the most economically viable when it comes to balancing factors like cost and rate of reaction
Compromise conditions
In this type of system, only energy—not matter—can be exchanged with the surroundings.
Closed system
This term describes the proportion of reactants that have been converted into products.
Extent of reaction
If a reaction has a K value of 1.3 x 10-8, the equilibrium position is said to favour these.
Reactants
Decreasing the volume of a gaseous system will cause the equilibrium to shift toward the side with this many particles.
Fewer gas particles
These unwanted reactions occur alongside the main reaction, reducing the yield of the desired product.
Side reactions
This state is reached when the rate of the forward reaction exactly equals the rate of the back reaction.
Dynamic equilibrium
These specific "harpoon" arrows are used in a chemical equation to represent a reversible reaction.
Bidirectional arrows
This mathematical ratio of products to reactants is used when a system has not yet reached equilibrium.
Reaction Quotient (Q)
For an exothermic reaction, an increase in temperature will cause the equilibrium to shift in this direction.
Left (Back reaction)
This Green Chemistry principle involves using substances to speed up a reaction without affecting the equilibrium position.
Catalysis
On a concentration-time graph, equilibrium is reached when the lines for all substances become this.
Constant/Horizontal
Unlike the rate of reaction, which measures change over time, the "extent" specifically refers to this.
The theoretical yield or the proportion of reactants converted
If the reaction quotient (Q) is greater than the equilibrium constant (K), the system will shift in this direction to reach equilibrium.
Left (Net back reaction)
Adding water to an aqueous equilibrium system (dilution) shifts the position toward the side with the...
Greater number of particles
Hydrogen sourced from Steam Methane Reforming (SMR) is often referred to by this colour-coded name due to its CO2 emissions.
Grey hydrogen
This type of table is used to calculate equilibrium concentrations using initial amounts and stoichiometry.
nICE table
This describes a reaction where once reactants are converted to products, they cannot be converted back.
Irreversible reaction
In the equilibrium expression for aW + bX ↔ cY + dZ, these parts of the chemical equation become the powers/exponents.
Stoichiometric coefficients
This principle states that a system at equilibrium will shift to partially oppose any change made to it.
Le Châtelier’s Principle
The production of "green ammonia" is integral to achieving this specific United Nations Sustainable Development Goal.
Goal 2 (Zero Hunger)
On a rate-time graph, the rate of the forward reaction does this as reactants are consumed.
Decreases