Integrated Rate Equations Flashcard

Front

What is the formula for calculating the half-life of a first-order reaction?

Back

The half-life (t1/2) of a first-order reaction is given by the formula: t1/2 = \frac{0.693}{k}, where k is the rate constant.

Front

How does the half-life of a first-order reaction change with varying initial concentration?

Back

The half-life of a first-order reaction is independent of the initial concentration.

Front

What is the relationship between the rate constant and half-life for a second-order reaction?

Back

For a second-order reaction, the half-life (t1/2) is given by the formula: t1/2 = \frac{1}{k[A]_0}, where k is the rate constant and [A]_0 is the initial concentration.

Front

If the initial concentration of a second-order reaction is doubled, how does the half-life change?

Back

The half-life of a second-order reaction will halve if the initial concentration is doubled.

Front

What is the unit of the rate constant (k) for a first-order reaction?

Back

The unit of the rate constant (k) for a first-order reaction is min^{-1}.

Front

What is the unit of the rate constant (k) for a second-order reaction?

Back

The unit of the rate constant (k) for a second-order reaction is L/(mol·s).

Front

How can you determine the order of a reaction from concentration vs. time graphs?

Back

For a first-order reaction, a plot of ln[A] vs. time will yield a straight line. For a second-order reaction, a plot of 1/[A] vs. time will yield a straight line.

Front

What is the integrated rate law for a first-order reaction?

Back

The integrated rate law for a first-order reaction is: ln[A] = -kt + ln[A]_0.

Front

What is the integrated rate law for a second-order reaction?

Back

The integrated rate law for a second-order reaction is: \frac{1}{[A]} = kt + \frac{1}{[A]_0}.

Front

What does a zero-order reaction imply about the concentration of reactants over time?

Back

In a zero-order reaction, the concentration of reactants decreases linearly over time.