The decomposition of XY is second order in XY and has a rate constant of 7.02 x 10^-3 M^-1 s^-1 at a certain temperature. How long will it take for the concentration of XY to decrease to 12.5% of its initial concentration when the initial concentration is 0.80 M?

For the hypothetical second-order reaction: A → products, the general rate law is: rate = k[A]^2. How long is the third half-life of the reaction if [A]0 is 0.080 M and the first half-life is 22 minutes?

In the reaction 3 BrO⁻(aq) → BrO₃⁻(aq) + 2 Br⁻(aq), a plot of 1/[BrO⁻] vs. time is linear. What does this indicate about the order of the reaction with respect to BrO⁻?

The decomposition of HI to H2 and I2 is a second-order reaction with a rate constant of 3.8 × 10⁻⁵ M⁻¹·s⁻¹ at a certain temperature. If the initial concentration of HI is 0.401 M, calculate the amount of time (in days) it will take to consume 70.8% of HI.

The decomposition of HI to H2 and I2 is a second-order reaction with a rate constant of 3.8 × 10⁻⁵ M⁻¹·s⁻¹ at a certain temperature. If the initial concentration of HI is 0.554 M, calculate the amount of time (in days) it will take to consume 72.4% of the initial concentration.

The reactant concentration in a first-order reaction was 7.30×10⁻² M after 25.0 s and 9.50×10⁻³ M after 95.0 s. What is the rate constant for this reaction?

The reactant concentration in a first-order reaction was 7.30 × 10^(-2) M after 25.0 s and 9.50 × 10^(-3) M after 95.0 s. What is the rate constant for this reaction?

Using the integrated rate law for a first-order reaction, ln[A]t = -kt + ln[A]0, how can you determine the rate constant (k) if you have concentration data over time?