- Is independent of initial concentration.
- Increases with increasing initial concentration.
- Decreases with increasing initial concentration.
- Is directly proportional to the rate constant.
No category found.
- Lowering of activation energy by temperature.
- Higher kinetic energy of molecules at higher temperature.
- Change in ?G with temperature.
- Shift in equilibrium with temperature.
- Elementary reactions only.
- Overall reactions based on experimental data.
- Reactions at equilibrium.
- Uncatalyzed reactions only.
- 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.
- 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.
- A decrease in intermolecular forces.
- A decrease in activation energy.
- An increase in the frequency of collisions.
- A change in the reaction mechanism.
- Negative of the slope.
- Positive of the slope.
- Y-intercept.
- X-intercept.
- 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.
- Formation over time.
- Disappearance over time.
- Equilibrium state.
- Constant concentration.
- It increases the activation energy of spoilage reactions.
- It shifts the equilibrium of spoilage reactions towards reactants.
- It provides more molecules with sufficient energy to react.
- It reduces the surface area of the food.
- Lowest activation energy.
- Fastest rate.
- Highest activation energy.
- Smallest number of molecules.
- 10 minutes.
- 15 minutes.
- 7.5 minutes.
- 30 minutes.
- Second order overall.
- Third order overall.
- Zero order with respect to Y.
- First order with respect to X.
- 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.
- 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.
