Given the reaction is first order.
So half life,t1/2=0.693/k
Where
K=rate constant=4.90*10^-4 min^-1
So t1/2=0.693/k =1414 min
The uncoiling of DNA is a first order reaction. Its activation energy is 420 kJ at...
6. The uncoiling of deoxyribonucleic acid (DNA) is a first order reaction with an activation energy of 420. kJ/mol. If the rate constant is 2.94 x 10-25-1 at 37°C, what is the rate constant when the temperature is decreased to 25°C?
. (a) If a first-order reaction has an activation energy of 104.6 kJ/mol and, in the equation k = k0 exp (-Ea/RT), k0 has a value of 5×1013/s, at what temperature will the reaction have a half-life of (i) 1 h; (ii) 1 day? [Note: the value of R is 8.314 kJ/kmol·K.] (b) If the sterilization of a biomaterial was heating at 121°C for 5 min, it could only be heated at 111°C due to the failure of the heating...
Could I get help on part B
3a. A certain first-order reaction is 35.5% complete in 4.90 minutes at 25°C. What is its rate constant e-kt K,=0.0895 min 64.5% min - 10 0.645 1.00 to = 8.95 x 100% 4.905 -0.0895 min 3b. If a first-order reaction has an activation energy of 104,600 J/mole and an A value of 5 x 10 sec !, at what temperature will the reaction have a half-life of 1 min? What about 30 days?
Consider an elementary first order reaction found to have an activation energy (EA) of 250 kJ/mole and a pre-exponential (A) of 1.7 x 1014 s–1. (a) Determine the rate constant at T = 750°C. (b) At what temperature will the reaction be three times as fast as at 750°C? (c) What fraction of the reaction will be completed in a batch reactor at 300°C over a period of 10 minutes?
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?
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)
Ethyl chloride vapor decomposes by the first-order reaction C2H5Cl→C2H4+HCl The activation energy is 249 kJ/mol and the frequency factor is 1.6×10^14 s^−1. A) Find the value of the specific rate constant at 710 K . B) Find the fraction of the ethyl chloride that decomposes in 20 minutes at this temperature. C) Find the temperature at which the rate of the reaction would be twice as fast.
1] The activation energy of an uncatalyzed reaction is 99 kJ/mol . The addition of a catalyst lowers the activation energy to 56 kJ/mol . a] Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 27 ∘C? Express the ratio to two significant digits. b] Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 139 ∘C?...