The rate constant, the activation energy and the arrhenius parameter of a chemical reaction at 25°C are 3 × 1014sec−1: 104.4Jmol−1 and 6.0 × 1014sec−1 respectively, the value of the rate constant as T → ∞ is:
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Activation energy is defined as the east possible every required for a reaction to take place. It is denoted by Ea and expressed as kJ/mol. It is dependent on temperature and catalyst.
Eg: Enzymes which are catalysts in our bodies lower activation Energy energy of many prourses so that the reaction can take place at a faster rate.
Given: Rate constant = 3 × 1014 sec–1
Activation anergy = 104.4 k smol–1
Arrhenius Parameter = 6.0 × 1014 sec–1
Arrhenius Equation: k= Ae–Ea/RT
when T→ ∞ the equation becomes
k = Ae–εa/R × ∞)
⇒ K = Ae–εa×0
⇒ K = Ae0 ⇒ K = A
⇒ k = 6.0 × 1014 sec–1
Answer →(B).
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