What is Integrated rate law equation?
=> [A] = -kt + [ A ] 0. The above equation is known as integrated rate equation for zero order reactions. We can observe the above equation as an equation of straight line with concentration of reactant on y-axis and time on x-axis. The slope of the straight line signifies the value of rate constant, k.
What is the purpose of the integrated rate law?
The integrated rate law gives the rate of a chemical reaction as a function of the initial concentration of one or more reactants after a specific period of time.
What is the difference between the rate law and the integrated rate law?
Rate laws can be expressed either as a differential rate law, describing the change in reactant or product concentrations as a function of time, or as an integrated rate law, describing the actual concentrations of reactants or products as a function of time.
What is the integrated rate equation for first order reaction?
For first-order reactions, the equation ln[A] = -kt + ln[A]0 is similar to that of a straight line (y = mx + c) with slope -k.
What are the variables in the integrated rate law?
Zero-Order Reactions
| Zero-Order | First-Order | |
|---|---|---|
| rate law | rate = k | rate = k[A] |
| units of rate constant | M s−1 | s−1 |
| integrated rate law | [ A ] = − k t + [ A ] 0 [ A ] = − k t + [ A ] 0 | ln [ A ] = − k t + ln [ A ] 0 ln [ A ] = − k t + ln [ A ] 0 |
| plot needed for linear fit of rate data | [A] vs. t | ln[A] vs. t |
How do you solve second order integrated rate law?
The integrated rate law for the second-order reaction A → products is 1/[A]_t = kt + 1/[A]_0. Because this equation has the form y = mx + b, a plot of the inverse of [A] as a function of time yields a straight line. The rate constant for the reaction can be determined from the slope of the line, which is equal to k.
What is the integrated rate equation for first-order reaction?
Which equation represents the integrated rate law for a zero order reaction?
Rate Laws from Graphs of Concentration Versus Time (Integrated Rate Laws)
| For a zero order reaction, | rate = k | (k = – slope of line) |
|---|---|---|
| For a 1st order reaction, | rate = k[A] | (k = – slope of line) |
| For a 2nd order reaction, | rate = k[A]2 | (k = slope of line) |
What is the integrated rate law for a zeroth order reaction?
The integrated rate law for the zero-order reaction A → products is [A]_t = -kt + [A]_0. Because this equation has the form y = mx + b, a plot of the concentration of A as a function of time yields a straight line. The rate constant for the reaction can be determined from the slope of the line, which is equal to -k.
How do you write an integrated rate law for a first-order reaction?
What is the integrated rate law for a 1st order reaction?
The integrated rate law for the first-order reaction A → products is ln[A]_t = -kt + ln[A]_0. Because this equation has the form y = mx + b, a plot of the natural log of [A] as a function of time yields a straight line.
What is the integrated rate equation for zero-order reaction?