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Answer :
The rate constant at 50°C is approximately 0.021 s⁻¹. The answer is a.
The Arrhenius equation relates the rate constant of a reaction to its activation energy and temperature:
[tex]k = Ae^{(-Ea/RT)[/tex]
where k is the rate constant, Ea is the activation energy, R is the gas constant (8.314 J/mol•K), T is the temperature in Kelvin, and A is the pre-exponential factor, which is a constant that depends on the specific reaction.
To find the rate constant at 50°C, we need to convert the temperature to Kelvin:
T = 50°C + 273.15 = 323.15 K
We can then use the Arrhenius equation and the given values to solve for the rate constant at 50°C:
[tex]k_2 = Ae^_(-Ea/RT_2)[/tex]
[tex]= (0.010 s^{-1})e^{(-35,800 J/mol / (8.314 J/mol•K * 323.15 K))[/tex]
= 0.021 s⁻¹
Therefore, the rate constant at 50°C is approximately 0.021 s⁻¹, which corresponds to option A.
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