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tekilochka [14]
2 years ago
9

The rate constant, k, for a reaction is 0.0354 sec1 at 40°C. Calculate the rate constant for the

Chemistry
1 answer:
deff fn [24]2 years ago
8 0

Answer:

The rate constant of the reaction at 125˚ is 0.3115 \ \text{sec}^{-1}.

Explanation:

The Arrhenius equation is a simple equation that describes the dependent relationship between temperature and the rate constant of a chemical reaction. The Arrhenius equation is written mathematically as

                                                  k \ = \ Ae^{\displaystyle\frac{-E_{a}}{RT}}

                                               \ln k \ = \ \ln A \ - \ \displaystyle\frac{E_{a}}{RT}

where k is the rate constant, E_{a} represents the activation energy of the chemical reaction, R is the gas constant, T is the temperature, and A is the frequency factor.

The frequency factor, A, is a constant that is derived experimentally and numerically that describes the frequency of molecular collisions and their orientation which varies slightly with temperature but this can be assumed to be constant across a small range of temperatures.

Consider that the rate constant be k_{1} at an initial temperature T_{1} and the rate constant k_{2} at a final temperature T_{2}, thus

                         \ln k_{2} \ - \ \ln k_{1} = \ \ln A \ - \ \displaystyle\frac{E_{a}}{RT_{2}} \ - \ \left(\ln A \ - \ \displaystyle\frac{E_{a}}{RT_{1}}\right) \\ \\ \\ \rule{0.62cm}{0cm} \ln \left(\displaystyle\frac{k_{2}}{k_{1}}\right) \ = \ \displaystyle\frac{E_{a}}{R}\left(\displaystyle\frac{1}{T_{1}} \ - \ \displaystyle\frac{1}{T_{2}} \right)

                                         \rule{1.62cm}{0cm} \displaystyle\frac{k_{2}}{k_{1}} \ = \ e^{\displaystyle\frac{E_{a}}{R}\left(\displaystyle\frac{1}{T_{1}} \ - \ \displaystyle\frac{1}{T_{2}} \right)} \\ \\ \\ \rule{1.62cm}{0cm} k_{2} \ = \ k_{1}e^{\displaystyle\frac{E_{a}}{R}\left(\displaystyle\frac{1}{T_{1}} \ - \ \displaystyle\frac{1}{T_{2}} \right)}

Given that E_{a} \ = \ 26.5 \ \ \text{kJ/mol}, R \ = \ 8.3145 \ \ \text{J mol}^{-1} \ \text{K}^{-1}, T_{1} \ = \ \left(40 \ + \ 273\right) \ K, T_{2} \ = \ \left(125 \ + \ 273\right) \ K, and k_{1} \ = \ 0.0354 \ \ \text{sec}^{-1}, therefore,

           k_{2} \ = \ \left(0.0354 \ \ \text{sec}^{-1}\right)e^{\displaystyle\frac{26500 \ \text{J mol}^{-1}}{8.3145 \ \text{J mol}^{-1} \ \text{K}^{-1}}\left(\displaystyle\frac{1}{313 \ \text{K}} \ - \ \displaystyle\frac{1}{398 \ \text{K}} \right)} \\ \\ \\ k_{2} \ = \ 0.3115 \ \ \text{sec}^{-1}                      

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Explanation:

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Protons are located at the center of atoms inside the nuclei. They cannot be gained or lost in chemical reactions. However, electrons are outside the nuclei and can be gained or lost. When an atom loses one or more electrons, it will carry more positive charge than negative charge. It will becomes a positive ion. Conversely, when an atom gains one or more electrons, it becomes a negative ion.

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This definition can be written as the acronym OILRIG. (Khan Academy.)

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Hope this helps :-)

Have a great rest of your day or night!

Enjoy your studies and assignments

<3 simplysun

ps. I do not own any of these answers so please don't give full credit to me

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