High School

Chapter 13: The rate constant for a reaction at 25°C is 0.010 s⁻¹, and its activation energy is 35.8 kJ/mol. What is the rate constant at 50°C?

A. 0.021 s⁻¹
B. 0.010 s⁻¹
C. 0.003 s⁻¹
D. 0.031 s⁻¹

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.

To know more about rate constant, refer here:
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