Advertisements
Advertisements
प्रश्न
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?
Advertisements
उत्तर
Given: k1 = 4.5 × 103 s−1
T1 = 273 + 10 = 283 K
k2 = 1.5 × 104 s−1
Ea = 60 kJ mol−1 = 6.0 × 104 J mol−1
T2 = ?
From Arrhenius equation, we obtain,
`log k_2/k_1 = E_a/(2.303 R)((T_2 - T_1)/(T_1T_2))`
⇒ log `(1.5 xx 10^4)/(4.5 xx 10^3) = (60000)/(2.303 xx 8.314) ((T_2 - 283) /(283 xx T_2))`
⇒ log 3.333 = `3133.63 (T_2 - 283)/(283 xx T_2)`
⇒ 0.5228 = `3133.63 (T_2 - 283)/(283 xx T_2)`
⇒ `0.5228/3133.63 = (T_2 - 283)/(283 xx T_2)`
⇒ 1.6683 × 10−4 = `(T_2 - 283)/(283 xx T_2)`
⇒ 1.6683 × 10−4 × 283 × T2 = T2 − 283
⇒ 0.0472 T2 = T2 − 283
283 = T2 − 0.0472 T2
283 = (1 − 0.0472) T2
283 = 0.9528 T2
⇒ T2 = `283/0.9528`
= 297 K
= 297 − 273
= 24°C
Hence, k would be 1.5 × 104 s−1 at 24°C.
Notes
The answer in the textbook is incorrect.
संबंधित प्रश्न
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?
In the Arrhenius equation for a first order reaction, the values of ‘A’ of ‘Ea’ are 4 × 1013 sec−1 and 98.6 kJ mol−1 respectively. At what temperature will its half life period be 10 minutes?
[R = 8.314 J K−1 mol−1]
What is the effect of adding a catalyst on Activation energy (Ea)
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 ?
Write a condition under which a bimolecular reaction is kinetically first order. Give an example of such a reaction. (Given : log2 = 0.3010,log 3 = 0.4771, log5 = 0.6990).
The rate of chemical reaction becomes double for every 10° rise in temperature because of ____________.
Activation energy of a chemical reaction can be determined by ______.
During decomposition of an activated complex:
(i) energy is always released
(ii) energy is always absorbed
(iii) energy does not change
(iv) reactants may be formed
Which of the following statements are in accordance with the Arrhenius equation?
(i) Rate of a reaction increases with increase in temperature.
(ii) Rate of a reaction increases with decrease in activation energy.
(iii) Rate constant decreases exponentially with increase in temperature.
(iv) Rate of reaction decreases with decrease in activation energy.
Oxygen is available in plenty in air yet fuels do not burn by themselves at room temperature. Explain.
Thermodynamic feasibility of the reaction alone cannot decide the rate of the reaction. Explain with the help of one example.
For an endothermic reaction energy of activation is Ea and enthalpy of reaction ΔH (both of there in KJ moI–1) minimum value of Ea will be ______.
The activation energy in a chemical reaction is defined as ______.
The activation energy in a chemical reaction is defined as ______.
The equation k = `(6.5 xx 10^12 "s"^(-1))"e"^(- 26000 " K"//"T")` is followed for the decomposition of compound A. The activation energy for the reaction is ______ kJ mol-1. (Nearest integer) (Given: R = 8.314 JK-1 mol-1)
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.
What happens to the rate constant k and activation energy Ea as the temperature of a chemical reaction is increased? Justify.
Activation energy of any chemical reactions can be calculated if one knows the value of:
Assertion (A): A reaction can have zero activation energy.
Reason (R): The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to the threshold value is called activation energy.
In the light of the above statements, choose the correct answer from the options given below:
