Integrated Rate Laws (2/3): Second Order Calculation

The video revisits a problem from a previous video, where the rate constant was determined assuming a first order reaction. It then calculates the rate constant assuming a second order reaction using the integrated rate law. The video explains the derivation of the units for a second order rate constant and concludes by highlighting the differences in rate constants due to different reaction orders. The next video will explore determining the true reaction order using additional data.

What was the initial concentration of reactant A in the problem discussed?

• 0.8 molar

• 0.6 molar

• 0.4 molar

• 0.2 molar

Which equation is used to calculate the rate constant for a second-order reaction?

• ln[A]t = ln[A]0 - kt

• Rate = k[A]

• Rate = k[A]^2

• 1/[A]t = 1/[A]0 + kt

What is the calculated second-order rate constant for the reaction?

• 0.0244 inverse molar inverse seconds

• 0.0741 inverse molar inverse seconds

• 0.0244 per second

• 0.0741 per second

How are the units for a second-order rate constant derived?

• By multiplying rate by concentration squared

• By dividing rate by concentration squared

• By multiplying concentration by time

• By dividing rate by concentration

What are the units for a second-order rate constant?

• Inverse molar per second

• Molar squared per second

• Molar per second

• Inverse molar inverse seconds