The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.
The time required for 10% completion of a first order reaction at 298 k is equal to that required for its 25% completion at 308 K. If the value of A is 4 × 1010 s-1, Calculate k at 318 k Read More …
The decomposition of A into product has value of k as 4.5 × 103 s-1 at 10°C and energy ofactivation 60 kJ mol-1. At what temperature would k be 1.5 × 104 s–1?
The rate constant for the first order decomposition of H2O2 is given by the following equation: log k = 14.34 – 1.25 × 104 K/T. Calculate Ea for this reaction and at what temperature will its half-period be 256 minutes?
The decomposition of hydrocarbon follows the equation k = (4.5× 1011 s-1) e-28000 k/T Calculate Ea
Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law with t1/2 = 3.00 hours. What fraction of sample of sucrose remains after 8 hours?
Consider a certain reaction A → Products with k = 2.0 × 10-2 s–1. Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L-1.
The rate constant for the decomposition of hydrocarbons is 2.418 × 10-5 s-1 at 546 k. If the energy of activation is 179.9 kJ /mol, what will be the value of pre-exponential factor.
The rate constant for the decomposition of N2O5 at various temperatures is given below:
The following data were obtained during the first order thermal decomposition of SO2Cl2 at a constant volume.
For the decomposition of azoisopropane to hexane and nitrogen at 543 k, the following data are obtained.