
6. The uncoiling of deoxyribonucleic acid (DNA) is a first order reaction with an activation energy...
The uncoiling of DNA is a first order reaction. Its activation energy is 420 kJ at 37degree C, the rate constant is 4.90 times 10^-4 min^-1. What is the half-life of the uncoiling if the organism has a temperature of 37degree C (104degreeF).
3) The rate constant of a first order reaction is 2.6 x 10+ s' at 255 °C. If the activation energy is 99.9 KJ/mol, calculate the temperature at which its rate constant is 4.8 x 104 sl.
if a first order reaction has an activation energy of 48.0 kj/mol and frequency factor of 2.4X10^6. what is the rate constant at 20.0*C and at 30.0*C?
A first order reaction is found to have an activation energy of 105.2 kJ mol-1 . If the rate constant for this reaction is 4.60 ×10-6s -1 at 275 K, and the initial reagent concentration is 2.50 mol L -1 , what is the remaining concentration after 500 seconds at a higher temperature of 325 K?
The following gas-phase reaction follows first-order kinetics. CIO2F======> CIOF+O The activation energy of this reaction is 186 kJ/mol. The value of k at 322°C is 6.76 x 10-4 S-1 . a. What would be the value of k for this reaction at room temperature, 25°C? k = _____ S-1 b. At what temperature would this reaction have a k value of ? Temperature = ______ oC
The following gas-phase reaction follows first-order kinetics. CIO2F======> CIOF+O The activation energy of this reaction is 186 kJ/mol. The value of k at 322°C is 6.76 x 10-4 S-1 . a. What would be the value of k for this reaction at room temperature, 25°C? k = _____ S-1 b. At what temperature would this reaction have a k value of 9.50 x 10-2 S-1 ? Temperature = ______ oC
2. The activation energy for the following first-order reaction is 102 kJ/mol. N2O(g) → 2NO(g) + 1/2O2(g) The value of the rate constant (k) is 1.35 x 10-s-1 at 35°C. What is the value of k at 20°C? (6 points)
12. The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 × 10−10 s−1 at 25°C. Calculate the rate constant at 52.1°C if the activation energy is 116 kJ/mol. _____ ×10^____ s−1 (Enter your answer in scientific notation.) 14. The rate constant of a first-order reaction is 2.75 × 10−4 s−1 at 350.°C. If the activation energy is 101 kJ/mol, calculate the temperature at which its rate constant...
Cyclopropane isomerizes to propylene according to a first order reaction: cyclopropane → propylene The activation energy is Ea=272 kJ/mol. At 773K, the reaction rate constant is 6.1 x 10-4 5-1 a. Calculate the pre-exponential factor, A, for this reaction b. Calculate the rate constant for this reaction at 298K.
A first order chemical reaction has an energy of activation of 90.0 kJ/mol and a rate constant of 0.0275 s-1 at 20oC. Find the rate constant for the chemical reaction at 50oC. R = 8.31447215 J/(mol×K)