Chemical Kinetics Quiz

The time it takes for the reactant concentration to decrease to half its initial value.

A reaction whose rate depends on the concentration of one reactant raised to the first power.

The half-life of a first-order reaction is constant throughout the reaction.

A reaction whose rate depends on the concentration of one reactant raised to the second power.

The half-life of a second-order reaction depends on the initial concentration.

The time it takes for the reactant in a second-order reaction to decrease to half its starting value.

The plot of 1/[A] versus time for a second-order reaction results in a straight line.

The slope of the straight line in the plot of 1/[A] versus time for a second-order reaction represents the rate constant (k).

A reaction where the rate is independent of the concentration of reactants. The rate law is Rate = k, where k is the rate constant and is a constant value.

The time it takes for the concentration of a reactant to decrease to half its initial value. This is a specific concept used for first-order reactions.

A graphical representation of the natural logarithm of concentration ([A]t) against time (t) for a first-order reaction. It yields a straight line with a slope of -k (the rate constant) and a y-intercept of ln[A]0 (the natural logarithm of the initial concentration).

The relationship between the rate constant (k) and temperature (T) of a reaction. It states that the rate constant increases exponentially with increasing temperature. The equation is k = A*exp(-Ea/RT), where A is the pre-exponential factor, Ea is the activation energy, and R is the gas constant.

The minimum amount of energy required for molecules to react. It's the energy barrier that must be overcome for a reaction to occur. It appears in the Arrhenius equation.

A plot used to determine the activation energy (Ea) of a reaction. It graphs the natural logarithm of the rate constant (ln k) against the reciprocal of the absolute temperature (1/T). The slope of this line is equal to -Ea/R.

The integrated rate law for a zero-order reaction relates the concentration of the reactant [A] at time t, [A]t, to the initial concentration [A]0 and the rate constant k.

For a zero-order reaction, the half-life continuously decreases with each subsequent half-life, making it half of the previous one.

A plot of concentration [A] versus time for a zero-order reaction yields a straight line with a negative slope. The slope of the line represents the rate constant (k), and the y-intercept represents the initial concentration [A]0.

The rate constant (k) is the negative of the slope of the concentration versus time plot in a zero-order reaction.

Determining the order of a reaction involves plotting concentration data versus time, then analyzing the linearity of the plots. If the concentration versus time plot is linear, the reaction is zero-order. If linear after conversion to ln[A] versus time, the reaction is first-order. If linear after conversion to 1/[A] versus time, the reaction is second-order.

Reactions occur faster at higher temperatures due to increased reactant collisions with sufficient energy and proper orientation.

This theory explains how reactions occur through successful collisions between reactant molecules. Successful collisions require sufficient energy (activation energy) and correct orientation of the colliding molecules.

The minimum energy reactants need to collide and form products.

A plot of the natural logarithm of the rate constant (ln k) versus the reciprocal of temperature (1/T). It is used to determine the activation energy (Ea) of a reaction.

A substance that speeds up a chemical reaction without being consumed itself, and is recovered unchanged at the end of the reaction.

The process of a catalyst providing an alternative pathway for a reaction with a lower activation energy, leading to a faster reaction rate.

A catalyst that exists in the same phase as the reactants, such as a catalyst that is in the same solution as the reactants.

A catalyst that exists in a different phase than the reactants. For example, a solid catalyst in a liquid reaction mixture.

The change in the rate constant of a reaction when the temperature is changed. This change is described by the Arrhenius equation.