Rate of reaction = -1/a delta[A]/delta t = - 1/b delta[B]/delta t = 1/c delta[C]/delta t...
Part A: The rate constant for a certain reaction is k = 2.30×10−3 s−1 . If the initial reactant concentration was 0.450 M, what will the concentration be after 3.00 minutes? Part B: A zero-order reaction has a constant rate of 4.10×10−4 M/s. If after 35.0 seconds the concentration has dropped to 5.50×10−2 M, what was the initial concentration? Express your answer with the appropriate units.
Most of the time, the rate of a reaction depends on the concentration of the reactant. In the case of second-order reactions, the rate is proportional to the square of the concentration of the reactant. Select the image to explore the simulation, which will help you to understand how second-order reactions are identified by the nature of their plots. You can also observe the rate law for different reactions. In the simulation, you can select one of the three different...
The rate constant for a certain reaction is k = 1.70×10−3 s−1 . If the initial reactant concentration was 0.900 M, what will the concentration be after 6.00 minutes? [A]t= B) A zero-order reaction has a constant rate of 3.90×10−4 M/s. If after 65.0 seconds the concentration has dropped to 4.00×10−2 M, what was the initial concentration? [A]0=
A plot of ln Rate vs. 1/T for a certain reaction gave a straight line with a slope of -8571. What is the activation energy for this reaction? Give your answer in kJ/mole please show work What is the order of reaction with respect to a certain reactant if doubling the concentration of that reactant causes the reaction rate to double? please explain What is the order of reaction with respect to a certain reactant if quadrupling the concentration of...
B) Determine the integrated rate law for this reaction. C) Calculate the half-life for this reaction. D) How much time is required for the concentration of A to decrease to 4.25x10^-3 M A certain reaction has the following general form: At a particular temperature and Alo 3.40 × 10-2 M concentration versus time data were collected for this reaction, and a plot of ln A versus time resulted in a straight line with a slope value of -2.91 x 10-2...
Part A: The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial reactant concentration was 0.150 M, what will the concentration be after 7.00 minutes? Part B: A zero-order reaction has a constant rate of 4.60×10−4 M/s. If after 30.0 seconds the concentration has dropped to 8.00×10−2 M, what was the initial concentration? Part C: A certain reaction has an activation energy of 60.0 kJ/mol and a frequency factor of A1 = 7.80×1012 M−1s−1...
The rate constant for a certain reaction is k = 5.20×10−3 s−1 . If the initial reactant concentration was 0.250 M, what will the concentration be after 10.0 minutes?
The rate constant for a certain reaction is k = 2.50×10−3 s−1 . If the initial reactant concentration was 0.950 M, what will the concentration be after 10.0 minutes?
The rate constant for a certain reaction is k = 5.50×10−3 s−1 . If the initial reactant concentration was 0.950 M, what will the concentration be after 14.0 minutes?
The rate constant for a certain reaction is k = 8.50×10−3 s−1 . If the initial reactant concentration was 0.150 M, what will the concentration be after 20.0 minutes?