The half-life of benzoyl peroxide at 65oC is 20 hours. Calculate the rate constant of decomposition of this initiator at this temperature.
The half-life of benzoyl peroxide at 65oC is 20 hours. Calculate the rate constant of decomposition...
The first-order decomposition of hydrogen peroxide has a half-life of 10.7 h at 20°C. a. What is the rate constant (expressed in hr−1) for this reaction? _____________ Write answer to three significant figures and NO UNITS in answer. b. If you started with a solution that was 7.5 × 10−3 M H2O2, what would be the concentration of H2O2 after 3.3 h? __________
For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at 25°C is 0.027 s-1. What is the rate constant at 45°C? For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at 25°C is 0.027 s-1. At what temperature will the rate constant be 35% greater than the rate constant at 25°C?
If the half-life for decomposition of a drug is 12 hours, how long (in hours) would it take for 500 mg of the drug to decompose by 10%? Assuming first order kinetics and at a constant temperature: (Assume must be numeric; round the final answer to the nearest WHOLE number)
How do you calculate the half life for this reaction? The first-order reaction of decomposition of azomethane is given below: At a certain temperature, the rate constant for this reaction equals 3.05 X 10^-3 s^-1. Calculate the half-life of this reaction (in seconds) at the same temperature.
3. The half-life for the first order decomposition of N2O3(g) is 6.00 104 s1 at 20 °C. a) Calculate the rate constant, k, at this temperature. b) What percentage of the N2Os molecules will have reacted after one hour?
The rate constant for the enzyme-catalysed decomposition of hydrogen peroxide, H2O2, increases by a factor of 3.8 when the temperature is increased from 298 K to 348 K. Determine the activation energy.
The rate law for a reaction is: rates = k[A]. Calculate the half-life of A, in hours, if the rate constant is 4.7 x 10-5 sec-1
For problem #3 and 4, a. b. C. Calculate the rate constant. Calculate half life Calculate the time it takes for the concentration to go down to 75% of its original value. 3. The rate law for the decomposition of phosphine (PH3) is: Rate k [PH3] It takes 120. S for 1.00 M PH3 to go down to 0.250 M
Rate constant for decomposition of hydrogen peroxide is 7.0 x10-5 s-1at 300.0K, with activation energy of 75 kJ/mol. At what temperature would the reaction rate be doubled?
Polymer chemistry If an initiator has a halt-life of 4h, what percentage of this initiator will remain after 12 h? Which is the better way to increase polymer production rates for free-radical reactions in general (a) increasing temperature or (b) increasing the initiator concentration and why? What is the limiting step in free-radical chain polymerization? What is the advantage of producing free-radicals by UV radiation instead of thermal energy? If [M] = 1 Times 10^-11 mol/L under steady-state conditions, what...