An energy profile for the reaction a⇌b (left), and the change in concentration of b as a function of time (right), with and without a catalyst. green curves show the reaction with a catalyst; black curves show the reaction without a catalyst. part a what quantity dictates the speed of a reaction? what quantity dictates the speed of a reaction? the energy difference between the initial state and the transition state the energy difference between the initial state and the final state

What quantity dictates the speed of a reaction? The activation energy

Explanation:

According to the collision theory, when molecules collide, they must overcome an energy barrier for the reaction to take place. This energy, known as activation energy, is represented by the difference in energy between the initial state and the transition state. The higher the activation energy, the slower the reaction. That's why catalysts reduce the activation energy to accelerate the reaction.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

the answer is minerals.