Chemical Kinetics

These flashcards cover key concepts in Chemical Kinetics, including rate laws, integrated rate equations, and the effects of temperature on reaction rates.

What does the integrated rate law show?

The relationship between concentration and time.

In a first-order reaction, how is the integrated rate law expressed?

ln[A]t = -kt + ln[A]0.

What is the slope of a first-order reaction plot of ln[A] vs. time?

The slope is -k.

How can you determine the rate constant from the graph of a first-order reaction?

The slope of the straight line is equal to -k.

What is the equation for rate in a second-order reaction?

Rate = k[A]^2.

What does the half-life of a reaction depend on?

The order of the reaction.

For a first-order reaction, what is the half-life formula?

t1/2 = 0.693/k.

In a first-order reaction, how does the concentration of the reactant change over time?

It decreases exponentially.

How is the rate constant, k, related to temperature in chemical kinetics?

It is dependent on temperature and described by the Arrhenius equation.

What is the Arrhenius equation?

k = Ae^(-Ea/(RT)).

What does Ea represent in the Arrhenius equation?

The activation energy required to start a reaction.

What effect does increasing temperature have on reaction rates?

It increases the reaction rate.

What does the frequency factor (A) represent in the Arrhenius equation?

The number of times reactants approach the activation energy per unit time.

What is the significance of the exponential factor in the Arrhenius equation?

It represents the fraction of molecules with sufficient energy to overcome the activation barrier.

How can you show that a reaction is first-order using experimental data?

By plotting the natural logarithm of the concentration vs. time and obtaining a straight line.

What happens to the concentration of a substance in a zero-order reaction?

It decreases linearly over time.