- Time.
- Concentration.
- Rate of reaction.
- Reciprocal of time.
No category found.
- Is constant throughout the reaction.
- Decreases as the reaction proceeds.
- Is lower than the instantaneous rate at the beginning of the interval.
- Is higher than the instantaneous rate at the end of the interval.
- The overall reaction.
- The slowest step of a reaction.
- Each elementary step of a reaction.
- The formation of products.
- Initial concentration of reactants.
- Temperature of the reaction.
- Order of the reaction.
- Activation energy.
- Zero-order reaction.
- First-order reaction.
- Second-order reaction.
- Reaction whose rate is decreasing.
- Halve.
- Double or triple.
- Remain unchanged.
- Quadruple.
- A straight line with positive slope.
- A straight line with negative slope.
- A curve with a constant slope.
- An exponentially decaying curve.
- Zero-order.
- First-order.
- Second-order.
- Third-order.
- Increase it.
- Decrease it.
- Have no effect.
- Increase it for exothermic reactions only.
- Decrease the rate by reducing molecular interactions.
- Increase the rate by increasing surface area.
- Have no effect on the rate.
- Increase the rate by changing the order of reaction.
- Rate=k[Reactant]n
- Rate=??t?[Reactant]?
- Rate=k
- Rate=?t?[Product]?
- The stoichiometry of the balanced chemical equation.
- The mechanism of the reaction.
- The overall enthalpy change.
- The total number of steps in the reaction.
- 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.
- 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.
- 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.
- 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.
