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The activation energy of the reaction at a given temperature is found to (2.303 RT) J mol-1. The ratio of rate constant to the Arrhenius factor is
- a)0.01
- b)0.1
- c)0.02
- d)0.001
Correct answer is option 'B'. Can you explain this answer?
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The activation energy of the reaction at a given temperature is found ...
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The activation energy of the reaction at a given temperature is found ...
The activation energy of a reaction is the minimum amount of energy required for a chemical reaction to occur. It can be determined experimentally by measuring the rate constant of the reaction at different temperatures and using the Arrhenius equation. The Arrhenius equation relates the rate constant (k) of a reaction to the temperature (T) and the activation energy (Ea) of the reaction.
The Arrhenius equation is given by:
k = A * exp(-Ea/RT)
Where:
k is the rate constant
A is the pre-exponential factor or the frequency factor
Ea is the activation energy
R is the gas constant (8.314 J/mol·K)
T is the temperature in Kelvin
The ratio of the rate constant to the Arrhenius factor is given by:
k/A = exp(-Ea/RT)
To find the ratio of the rate constant to the Arrhenius factor, we need to express the activation energy in terms of RT. Given that the activation energy is (2.303 RT) J/mol, we can rewrite it as:
Ea = 2.303 RT
Substituting this value into the equation, we have:
k/A = exp(-(2.303 RT)/RT)
Simplifying the equation, we get:
k/A = exp(-2.303)
Since the exponential function e^(-2.303) is approximately equal to 0.1, we can conclude that:
k/A ≈ 0.1
Therefore, the correct answer is option 'B' - 0.1. The ratio of the rate constant to the Arrhenius factor is approximately 0.1.
The Arrhenius equation is given by:
k = A * exp(-Ea/RT)
Where:
k is the rate constant
A is the pre-exponential factor or the frequency factor
Ea is the activation energy
R is the gas constant (8.314 J/mol·K)
T is the temperature in Kelvin
The ratio of the rate constant to the Arrhenius factor is given by:
k/A = exp(-Ea/RT)
To find the ratio of the rate constant to the Arrhenius factor, we need to express the activation energy in terms of RT. Given that the activation energy is (2.303 RT) J/mol, we can rewrite it as:
Ea = 2.303 RT
Substituting this value into the equation, we have:
k/A = exp(-(2.303 RT)/RT)
Simplifying the equation, we get:
k/A = exp(-2.303)
Since the exponential function e^(-2.303) is approximately equal to 0.1, we can conclude that:
k/A ≈ 0.1
Therefore, the correct answer is option 'B' - 0.1. The ratio of the rate constant to the Arrhenius factor is approximately 0.1.
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The activation energy of the reaction at a given temperature is found ...
Option B : 0.1
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The activation energy of the reaction at a given temperature is found to (2.303 RT) J mol-1. The ratio of rate constant to the Arrhenius factor isa)0.01b)0.1c)0.02d)0.001Correct answer is option 'B'. Can you explain this answer?
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