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The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K. The activation energy of the reaction is 255 kJ/mol. What would be the value of the rate constant at 9.50×102 K?

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sebassandin

Answer:

[tex]k_2=1.379x10^{-2}s^{-1}[/tex]

Explanation:

Hello.

In this case, for a normal reaction, when we know the rate constant at a determined temperature, we can compute at another temperature via the Arrhenius equation specified for temperature change:

[tex]k_2=k_1exp[-\frac{Ea}{R}(\frac{1}{T_2}-\frac{1}{T_1} )][/tex]

In such a way, the rate constant at 9.50x10² K is:

[tex]k_2=3.241x10^{-5}s^{-1}exp[-\frac{255000}{8.314}(\frac{1}{950}-\frac{1}{800} )]\\\\k_2=1.379x10^{-2}s^{-1}[/tex]

Best regards!

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