- Its overall order.
- The number of reactant molecules involved in that single step.
- The number of product molecules formed.
- Its dependence on temperature.
Category: Chemistry
- Collisions become more energetic.
- The activation energy decreases.
- The concentration of reactants increases.
- The gas molecules become more reactive.
- Equal to B.
- Double that of B.
- Half that of B.
- Cannot be determined from rate data.
- Rate constant.
- Frequency factor.
- Activation energy.
- Enthalpy change.
- All steps proceed at the same rate.
- The activation energy of the slowest step is the highest.
- The activation energy of the slowest step is the lowest.
- Reactants are consumed only in the slowest step.
- The stoichiometry of the overall balanced equation.
- The stoichiometric coefficients of the reactants in the fastest step.
- The molecularity of the rate-determining step.
- Experimental data.
- Catalyst (by providing ions).
- Inhibitor.
- Reactant.
- Surface area modifier.
- Concentration.
- Volume.
- Temperature.
- Pressure.
- Is independent of initial concentration.
- Increases with increasing initial concentration.
- Decreases with increasing initial concentration.
- Is directly proportional to the rate constant.
- Elementary reactions only.
- Overall reactions based on experimental data.
- Reactions at equilibrium.
- Uncatalyzed reactions only.
- Lowering of activation energy by temperature.
- Higher kinetic energy of molecules at higher temperature.
- Change in ?G with temperature.
- Shift in equilibrium with temperature.
- Rate = k[A][B]
- Rate = k[A]2[B]
- Rate = k[A][B]2
- Rate = k[A]2[B]2
- Its activation energy increases.
- It undergoes denaturation.
- Its substrate concentration decreases.
- It becomes more specific.
- The activation energy.
- The fraction of effective collisions.
- The frequency of collisions with proper orientation.
- The rate constant at infinite temperature.
- A decrease in intermolecular forces.
- A decrease in activation energy.
- An increase in the frequency of collisions.
- A change in the reaction mechanism.
- Any collision that occurs.
- Collisions with sufficient energy to break bonds.
- Collisions with correct orientation, regardless of energy.
- Collisions with both sufficient energy and proper orientation.
- Summing the stoichiometric coefficients of reactants.
- The highest exponent in the rate law.
- Summing the exponents of the concentration terms in the rate law.
- The molecularity of the slowest step.
- Negative of the slope.
- Positive of the slope.
- Y-intercept.
- X-intercept.
- Formation over time.
- Disappearance over time.
- Equilibrium state.
- Constant concentration.
