- Zero.
- First.
- Second.
- Third.
Category: Chemistry
- How exothermic the reaction is.
- How endothermic the reaction is.
- The energy barrier that must be overcome for the reaction to proceed.
- The spontaneity of the reaction.
- Decreasing the total number of collisions.
- Increasing the kinetic energy of molecules, making more collisions effective.
- Only increasing the number of collisions, not their energy.
- Changing the orientation of molecules.
- Increasing the temperature of the reaction.
- Directly increasing the concentration of reactants.
- Binding reactants to their active sites and lowering activation energy.
- Shifting the equilibrium to favor product formation.
- The rate is independent of that reactant's concentration.
- The reactant is not involved in the rate-determining step.
- Increasing that reactant's concentration will decrease the rate.
- Both A and B are correct.
- To shift it towards products.
- To shift it towards reactants.
- To make it more difficult to achieve.
- No effect, only affects the rate at which equilibrium is reached.
- Rate constant.
- Half-life.
- Order of reaction.
- Activation energy.
- An increase in temperature.
- A decrease in reactant concentrations.
- The formation of a catalyst.
- An increase in surface area.
- Changes with concentration but not temperature.
- Changes with temperature but not concentration.
- Changes with both temperature and concentration.
- Is always a whole number.
- Higher than the uncatalyzed reaction.
- Lower than the uncatalyzed reaction.
- Unchanged compared to the uncatalyzed reaction.
- Absent.
- The reaction is exothermic.
- The reaction is endothermic.
- Energy is required to overcome the reaction barrier.
- The reaction proceeds spontaneously.
- A decrease due to molecular instability.
- An increase due to reduced activation energy.
- An increase due to more frequent and more energetic collisions.
- No significant change.
- Speed only.
- Orientation only.
- Both proper orientation and sufficient energy.
- Minimal energy.
- Concentration.
- Surface area.
- Nature.
- Temperature.
- Activation energy is reduced.
- The concentration of gaseous reactants effectively increases.
- The equilibrium shifts to the product side.
- The temperature of the system rises.
- Elementary step.
- Overall step.
- Rate-determining step.
- Initiation step.
- Zero-order.
- First-order.
- Second-order.
- Third-order.
