Chemical Kinetics Quiz

The study of reaction rates and how they are influenced by various factors like concentration, temperature, and catalysts.

The study of the detailed step-by-step process by which a reaction occurs. It helps understand how reactions happen and how to control them.

The rate of a reaction is influenced by the concentration of reactants. Higher concentration means more frequent collisions between molecules, leading to a faster reaction.

Increasing temperature speeds up reactions by increasing the frequency of collisions between molecules and also providing more energy for these collisions to overcome activation energy.

Catalysts are substances that speed up reaction rates without being consumed in the process. They provide an alternative reaction pathway with lower activation energy.

The rate of a reaction for a gas will increase with increasing pressure. This is similar to how the rate of a reaction is affected by the concentration of reactants.

The rate of a reaction is directly proportional to the surface area of the reactants. A larger surface area leads to more frequent collisions, making the reaction faster.

For a reaction to occur, molecules must collide with the correct orientation. The more complex the molecules, the less likely they are to collide with the right orientation.

The rate of a reaction is affected by the speed of the molecules involved. Molecules with higher speeds, due to higher temperatures, collide more frequently and with more energy, increasing the rate of the reaction.

The energy barrier that reactants must overcome to form products. The minimum amount of energy required for a reaction to occur.

Most molecules at room temperature do not have enough energy to overcome the activation energy and react. Only a small fraction of molecules have enough energy to participate in the reaction.

The minimum amount of energy molecules must have to be able to collide effectively and form products. The molecules must have enough energy to break existing bonds and form new ones.

The state where reactants are in the process of transitioning to products. It is a high-energy, unstable state that quickly breaks down to form products.

A measure of the rate at which molecules move. The higher the temperature, the faster the molecules move.

The average kinetic energy of the molecules in a substance. This energy is directly proportional to the temperature of the substance. Higher temperatures result in higher average kinetic energy and faster molecule motion.

A constant in the Arrhenius equation that represents the rate constant at infinite temperature or when the activation energy is zero. It signifies the frequency of collisions between molecules.

The energy required for a collision between molecules to result in a reaction. It represents the minimum energy molecules need to overcome the energy barrier and react.

The fraction of molecules with enough energy to overcome the activation energy and react. It increases with temperature.

A substance that increases the rate of a chemical reaction without being consumed itself. It provides an alternative reaction pathway with lower activation energy.

Catalysts work by providing a lower activation energy pathway for the reaction, effectively lowering the energy barrier.

Catalysts do not alter the equilibrium position of a reaction, they only increase the rate at which equilibrium is reached.

Catalysts cannot make an unfavorable reaction (where energy is required) favorable. They can only speed up the reaction.

The standard free energy change (ΔG) of a reaction is not affected by a catalyst. Only the rate at which equilibrium is reached is changed.

The distribution of molecular energies in a gas, showing the proportion of molecules with different kinetic energies. Molecules with energies above a certain threshold (activation energy) can react.

Increasing temperature shifts the Maxwell-Boltzmann distribution to the right, meaning more molecules have enough energy to react. This is why reactions speed up at higher temperatures.

The mathematical equation that relates the rate constant (k) of a reaction to the activation energy (Ea), temperature (T), and the pre-exponential factor (A).

A constant that relates the rate of a chemical reaction to the concentration of reactants. It's a measure of how fast a reaction progresses.

The time required for the concentration of a reactant to decrease by half. It's a measure of how fast a reaction proceeds.

The time taken for a substance to lose 90% of its initial concentration. It's commonly used to assess the shelf-life of pharmaceuticals.

It is the graphical representation of the relationship between the rate constant (k) and temperature as implied by the Arrhenius equation. It is useful for determining the activation energy (Ea) of a reaction.

A catalyst is a substance that speeds up a reaction without being consumed in the process. It accomplishes this by lowering the activation energy of the reaction.

The rate of a reaction is directly proportional to the concentration of the reactant raised to the power of its order. For example, if the order is 2, doubling the concentration quadruples the rate.

The sum of the exponents of each reactant concentration in the rate law. It indicates the overall sensitivity of the reaction rate to changes in reactant concentrations.

The rate of a reaction is independent of the concentration of the reactant; it remains unchanged regardless of the reactant's concentration.

The rate of a reaction is directly proportional to the concentration of the reactant. Doubling the concentration doubles the rate.

The rate of a reaction is proportional to the square of the reactant concentration. Doubling the concentration quadruples the rate.

The sum of the exponents in the rate law for a reaction. It indicates the overall dependence of the reaction rate on the concentration of all reactants.

Reactions that occur in a single step. The molecularity of the reaction is equal to the order of the reaction.

The slowest step in a reaction mechanism. It determines the overall rate of the reaction. The rate of the reaction cannot exceed the rate of the slowest step.

A chemical reaction that involves the collision of two reactant molecules. The rate of the reaction is proportional to the product of the concentrations of the two reactants.

A chemical reaction that involves the collision of only one reactant molecule. The rate of the reaction is proportional to the concentration of the reactant.

A step in a reaction mechanism that involves the breaking of a bond within a molecule. The rate of the reaction is proportional to the concentration of the reactant.