Multiple Choice
For the reaction A → B, the rate constant is 0.0837 M–1•sec–1. How long would it take for [A] to decrease by 85%?
15. Chemical Kinetics
Integrated Rate Law
Back15. Chemical Kinetics
Integrated Rate Law
- Multiple Choice
The following reaction has a rate constant of 3.7 × 10–3 M•s–1 at 25°C:
A → B + C
Calculate the concentration of C after 2.7 × 10–3 sec where [A]0 was 0.750 M at 25°C; assume [C]0 = 0 M.
- Multiple Choice
For the decomposition of urea, NH2CONH2 (aq) + H+(aq) + 2 H2O (l) → 2 NH4+ (aq) + HCO3– (aq), the rate constant is 3.24 × 10–4 s–1 at 35°C. The initial concentration of urea is 2.89 mol/L. What fraction of urea has decomposed after 3.5 minutes?
- Multiple Choice
Iodine-123 is used to study thyroid gland function. As this radioactive isotope breaks down, after 5.7 hrs the concentration of iodine-123 is 56.3% complete. Find the rate constant of this reaction.
- Open Question
For the reaction x ⟶ y identify what the graphs of [x] versus time and [y] versus time would look like for various orders. in each graph, [?] represents either [x] or [y].
- Open Question
Consider the following general reaction and data: 2a + 2 b + c → d + 3 e
- Multiple ChoiceFor the reaction 2N2O5(g) → 4NO2(g) + O2(g) with a rate constant k = 2.8×10⁻³ sec⁻¹, if the initial concentration of [N2O5] is 1.58 mol/L, what is the concentration of N2O5 after 300 seconds?
- Multiple ChoiceFor 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?
- Multiple ChoiceIn 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⁻?
- Multiple ChoiceThe 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.
- Multiple ChoiceThe 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.
- Multiple ChoiceThe 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?
- Multiple ChoiceThe 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?
- Multiple ChoiceThe 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?
- Multiple ChoiceUsing 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?