equalibrium

What is collision theory?

Collision theory states that for a reaction to occur, particles must collide with sufficient energy and proper orientation.

How does surface area affect reaction rate?

A larger surface area increases the number of particles available to collide, leading to more frequent successful collisions and a faster reaction rate.

What is the difference between a 2 M and a 6 M solution of HCl?

A 6 M solution has more moles of HCl per liter than a 2 M solution, leading to a higher concentration of reactant particles and a faster reaction rate.

What factors can prevent a reaction from occurring despite collisions?

Factors include insufficient energy to break bonds, unfavorable temperature, low concentration of reactants, or inadequate surface area.

What is activation energy (Ea)?

Activation energy is the minimum energy required for reactants to collide successfully and form products.

What does a catalyst do?

A catalyst lowers the activation energy of a reaction, increasing the rate of reaction by providing an alternative pathway for the reaction.

What two conditions must be true for a collision to be effective?

The colliding particles must have sufficient energy and the correct orientation.

How does temperature affect reaction rates?

Increasing temperature raises the energy of particles, causing them to move faster and collide more frequently, which increases the reaction rate.

How does concentration affect reaction rates?

Higher concentration means more particles in a given volume, leading to a greater chance of successful collisions and a faster reaction rate.

What does Le Chatelier's Principle state?

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will shift in a direction that counteracts the disturbance.

What happens to equilibrium when temperature is increased?

If the reaction is endothermic, the equilibrium will shift to the right (toward products). If exothermic, it will shift to the left (toward reactants).

What is the effect of adding a common ion to a solution at equilibrium?

Adding a common ion shifts the equilibrium to the left, decreasing the concentration of the ion that was added.

What does it mean if K > 1?

If K > 1, the products are favored at equilibrium, indicating a greater concentration of products than reactants.

What does it mean if K < 1?

If K < 1, the reactants are favored at equilibrium, indicating a greater concentration of reactants than products.

What is the relationship between K and Q?

K is the equilibrium constant, while Q is the reaction quotient. If Q < K, the reaction will shift to the right; if Q > K, it will shift to the left.

What is an endothermic reaction?

An endothermic reaction absorbs heat from the surroundings, resulting in a positive ΔH.

What is an exothermic reaction?

An exothermic reaction releases heat to the surroundings, resulting in a negative ΔH.

How does pressure affect equilibrium?

Increasing pressure shifts the equilibrium toward the side with fewer moles of gas, while decreasing pressure shifts it toward the side with more moles of gas.

What is the effect of removing heat from an endothermic reaction?

Removing heat shifts the equilibrium to the left, favoring the reactants.

What is the effect of adding heat to an exothermic reaction?

Adding heat shifts the equilibrium to the left, favoring the reactants.

What does it mean for a reaction to reach equilibrium?

At equilibrium, the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

What is the significance of a reaction coordinate diagram?

A reaction coordinate diagram illustrates the energy changes during a reaction, including activation energy and the energy of reactants and products.

What does a higher concentration of reactants imply for the reaction rate?

A higher concentration of reactants increases the likelihood of collisions, thus speeding up the reaction.

What is the role of a catalyst in a reaction coordinate diagram?

A catalyst lowers the peak of the activation energy barrier in the reaction coordinate diagram, facilitating faster reactions.