How Does Temperature Affect the Rate Constant of a Reaction?

[phys1618]

Rate constant "answer check"

Homework Statement

given that activation energy for a certain reaction is 48 kJ/mol, and the rate constanct is 2.5 x 10^-2 s^-2 at 15 degrees Celsius. waht is the rate constant at 37 degrees Celsius?

Homework Equations

ln k1/k2 = [Ea/R] [(T1-T20)/(T1*T2)]

The Attempt at a Solution

my answer is k1= .1037740579 = .104 s^-1


thank you for all the help!

 

[sandbanana]

Converting all temperatures to absolute and 48kJ to 48000 J so the units on the gas constant cancel I came up with 5.3*10^-3 s^-2

I used this equation:

ln k1/ln k2 = Ea/R(1/T2-1/T1)

 

[Blueshift5]

I would like to provide some feedback on your attempt at solving this problem. First, your solution is correct in terms of the numerical value, but it would be better to express it in scientific notation (1.04 x 10^-1 s^-1) to maintain proper significant figures.

Secondly, it would be helpful to include units in your final answer. The rate constant is typically expressed in units of s^-1, so your final answer would be 1.04 x 10^-1 s^-1 at 37°C.

Lastly, it is important to mention that the equation you used, ln k1/k2 = [Ea/R] [(T1-T20)/(T1*T2)], is known as the Arrhenius equation and is used to calculate the rate constant at different temperatures. This equation assumes that the reaction follows the Arrhenius law and that the rate constant is dependent on temperature. However, there may be other factors that can affect the rate constant, such as changes in the reaction mechanism or the presence of catalysts. Therefore, it is always important to consider the limitations of the Arrhenius equation and to verify the result with experimental data.