Advertisements
Advertisements
प्रश्न
What happens to the rate constant k and activation energy Ea as the temperature of a chemical reaction is increased? Justify.
Advertisements
उत्तर
As the temperature of a chemical reaction rises, the rate constant k rises and the activation energy Ea falls.
According to Arrhenius equation
k = `"Ae"^(-"E"_"a"//"RT")`
As a result, the rate constant k rises exponentially as the temperature rises.
APPEARS IN
संबंधित प्रश्न
The rate constant for the first-order decomposition of H2O2 is given by the following equation:
`logk=14.2-(1.0xx10^4)/TK`
Calculate Ea for this reaction and rate constant k if its half-life period be 200 minutes.
(Given: R = 8.314 JK–1 mol–1)
The decomposition of A into product has value of k as 4.5 × 103 s−1 at 10°C and energy of activation 60 kJ mol−1. At what temperature would k be 1.5 × 104 s−1?
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 rate constant of a first order reaction are 0.58 S-1 at 313 K and 0.045 S-1 at 293 K. What is the energy of activation for the reaction?
The decomposition of a hydrocarbon has value of rate constant as 2.5×104s-1 At 27° what temperature would rate constant be 7.5×104 × 3 s-1if energy of activation is 19.147 × 103 J mol-1 ?
Predict the main product of the following reactions:
What happens to most probable kinetic energy and the energy of activation with increase in temperature?
Arrhenius equation can be represented graphically as follows:
The (i) intercept and (ii) slope of the graph are:
The decomposition of N2O into N2 and O2 in the presence of gaseous argon follows second-order kinetics, with k = (5.0 × 1011 L mol−1 s−1) `"e"^(-(29000 "K")/"T")`. Arrhenius parameters are ______ kJ mol−1.
The rate of a reaction quadruples when temperature changes from 27°C to 57°C calculate the energy of activation.
(Given: R = 8. 314 J K−1 mol−1, log 4 = 0.6021)
