1.What is the half-life for a particular reaction if the rate law is rate = (891 min⁻¹)[A]? 2. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.380 M? (k = 0.456 M⁻¹ s⁻¹) 3. What is the concentration of a reactant after 26.0 s if the initial concentration is 0.150 M and the rate constant is 5.4 x 10⁻² s⁻¹?
1.What is the half-life for a particular
2. A reaction was shown to follow second-order kinetics. How much time is required for [A] to change from 0.500 M to 0.380 M? (k = 0.456 M⁻¹ s⁻¹)
3. What is the concentration of a reactant after 26.0 s if the initial concentration is 0.150 M and the rate constant is 5.4 x 10⁻² s⁻¹?
4. The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.233 M. What is the value of k for this reaction?
5. a) Chemists graph kinetic data to determine rate constants and the order of reactions. Analyze this data. If the slope is -0.0170 for this reaction, determine the rate constant, k, for this reaction.
b) Given that k is 0.0017 s⁻¹ and the [A] is 0.1000 M, determone the rate for this reaction based on the rate law determined.
6. a) The kinetics of a gas phase reaction of the form A → Products results in a rate constant of 1.308 M⁻¹ s⁻¹. For this reaction, the initial concentration of A is 0.129 M. What is the half-life for this reaction?
b) The kinetics of a gas phase reaction of the form A → Products results in a rate constant of 1.308 M⁻¹ s⁻¹. For this reaction, the initial concentration of A is 0.129 M. What is the concentration of A after 0.385 seconds?
c) The kinetics of a gas phase reaction of the form A → Products results in a rate constant of 1.308 M⁻¹ s⁻¹. For this reaction, the initial concentration of A is 0.129 M. At what time would the concentration of A reach 0.042 M?
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
