- Second order overall.
- Third order overall.
- Zero order with respect to Y.
- First order with respect to X.
Category: Chemistry
- 10 minutes.
- 15 minutes.
- 7.5 minutes.
- 30 minutes.
- Solubility of reactants.
- Surface area of the catalyst.
- Pressure of the system.
- pH of the medium.
- A higher activation energy.
- The formation of a new, stable intermediate.
- A lower activation energy.
- A change in the overall enthalpy of reaction.
- Is independent of the initial concentration.
- Increases with increasing initial concentration.
- Decreases with increasing initial concentration.
- Is directly proportional to the rate constant.
- Time.
- Concentration.
- Rate of reaction.
- Reciprocal of time.
- First-order with respect to that reactant.
- Second-order with respect to that reactant.
- Zero-order with respect to that reactant.
- Catalyzed by that reactant.
- 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.
- Zero-order reaction.
- First-order reaction.
- Second-order reaction.
- Reaction whose rate is decreasing.
- Initial concentration of reactants.
- Temperature of the reaction.
- Order of the reaction.
- Activation energy.
- 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.
- Increase it.
- Decrease it.
- Have no effect.
- Increase it for exothermic reactions only.
- Zero-order.
- First-order.
- Second-order.
- Third-order.
- 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.
- The stoichiometry of the balanced chemical equation.
- The mechanism of the reaction.
- The overall enthalpy change.
- The total number of steps in the reaction.
- Rate=k[Reactant]n
- Rate=??t?[Reactant]?
- Rate=k
- Rate=?t?[Product]?
