Question

Chemical reaction A → B + C is zero order in A with a rate constant of 2.12 x 10 mol/Les at 25°C. a. Write the integrated rate law. b. Calculate the time for the concentration to reach 35% of the original. c. Determine the time for 85% of the original concentration to be consumed.

Answer 1

The integrated rate law for a zero-order reaction is [A] = [A]_0 - kt. To calculate the time for the concentration to reach 35% of the original, rearrange the equation. To determine the time for 85% of the original concentration to be consumed, substitute [A] = 0.15[A]_0 into the equation.

Step-by-step explanation:

The integrated rate law for a zero-order reaction is expressed as:

$$[A] = [A]_0 - kt$$

Where [A] is the concentration of reactant A at a given time, [A]_0 is the initial concentration of reactant A, k is the rate constant, and t is the time elapsed.

To calculate the time for the concentration to reach 35% of the original, you can rearrange the integrated rate law equation to solve for t when [A] = 0.35[A]_0:

$$t = \frac{[A]_0 - [A]}{k}$$

Finally, to determine the time for 85% of the original concentration to be consumed, you can substitute [A] = 0.15[A]_0 into the rearranged integrated rate law equation and solve for t:

$$t = \frac{[A]_0 - [A]}{k}$$