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The activation energy of a reaction is 50 kJ mol-1 and the value of rate constant at 300 K is 2.5 × 10-5 sec-1. What is the value of the frequency factor, A?
- a)4228.53 s-1
- b)3829.69 s-1
- c)7596.45 s-1
- d)6565.35 s-1
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
The activation energy of a reaction is 50 kJ mol-1 and the value of ra...
X 10^-4 s^-1. Calculate the rate constant at 350 K.
We can use the Arrhenius equation to calculate the rate constant at a different temperature:
k = A * e^(-Ea/RT)
where:
k = rate constant
A = pre-exponential factor
Ea = activation energy (50 kJ mol^-1 in this case)
R = gas constant (8.314 J mol^-1 K^-1)
T = temperature
We can solve for A by rearranging the equation:
A = k / e^(-Ea/RT)
Substituting in the values given at 300 K:
k = 2.5 x 10^-4 s^-1
Ea = 50 kJ mol^-1
R = 8.314 J mol^-1 K^-1
T = 300 K
A = (2.5 x 10^-4 s^-1) / e^(-50,000 J mol^-1 / (8.314 J mol^-1 K^-1 * 300 K))
A = 1.68 x 10^15 s^-1
Now, we can use this value of A and the Arrhenius equation to calculate the rate constant at 350 K:
k = A * e^(-Ea/RT)
k = (1.68 x 10^15 s^-1) * e^(-50,000 J mol^-1 / (8.314 J mol^-1 K^-1 * 350 K))
k = 1.14 x 10^-3 s^-1
Therefore, the rate constant at 350 K is 1.14 x 10^-3 s^-1.
We can use the Arrhenius equation to calculate the rate constant at a different temperature:
k = A * e^(-Ea/RT)
where:
k = rate constant
A = pre-exponential factor
Ea = activation energy (50 kJ mol^-1 in this case)
R = gas constant (8.314 J mol^-1 K^-1)
T = temperature
We can solve for A by rearranging the equation:
A = k / e^(-Ea/RT)
Substituting in the values given at 300 K:
k = 2.5 x 10^-4 s^-1
Ea = 50 kJ mol^-1
R = 8.314 J mol^-1 K^-1
T = 300 K
A = (2.5 x 10^-4 s^-1) / e^(-50,000 J mol^-1 / (8.314 J mol^-1 K^-1 * 300 K))
A = 1.68 x 10^15 s^-1
Now, we can use this value of A and the Arrhenius equation to calculate the rate constant at 350 K:
k = A * e^(-Ea/RT)
k = (1.68 x 10^15 s^-1) * e^(-50,000 J mol^-1 / (8.314 J mol^-1 K^-1 * 350 K))
k = 1.14 x 10^-3 s^-1
Therefore, the rate constant at 350 K is 1.14 x 10^-3 s^-1.
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Community Answer
The activation energy of a reaction is 50 kJ mol-1 and the value of ra...
Given,
Ea = 50 kJ mol-1
T = 300 K
k = 1.5 × 10-5 sec-1
R = 8.314 J K-1 mol-1
log k = – Ea / (2.303 RT) + log A
OR
log A = log k + Ea / (2.303 RT)
log A = log (1.5 × 10-5) + 50000 / (2.303 × 8.314 × 300)
log A = 3.88061
A = antilog (3.880611)
A = 7596.45 s-1.
Ea = 50 kJ mol-1
T = 300 K
k = 1.5 × 10-5 sec-1
R = 8.314 J K-1 mol-1
log k = – Ea / (2.303 RT) + log A
OR
log A = log k + Ea / (2.303 RT)
log A = log (1.5 × 10-5) + 50000 / (2.303 × 8.314 × 300)
log A = 3.88061
A = antilog (3.880611)
A = 7596.45 s-1.
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The activation energy of a reaction is 50 kJ mol-1 and the value of rate constant at 300 K is 2.5 × 10-5 sec-1. What is the value of the frequency factor, A?a)4228.53 s-1b)3829.69 s-1c)7596.45 s-1d)6565.35 s-1Correct answer is option 'C'. Can you explain this answer?
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