Calculating Activation Energy and Rate Constant for a Chemical Reaction

[kittymaniac84]

[SOLVED] Activation energy

The reaction, 2NOCI (g) = 2NO (g) + Cl^{}_2{}(g) , has rate constant values for the reaction of NOCl of 9.3 x 10^-6 Is at 350 K and 6.9 x 10^-4 Is at 400 K. Calculate the activation energy for the reaction. What is the rate constant at 425 K?

I am unsure how to solve this. Can someone help me and show me how to do it.

 

[gravenewworld]

SCREAMS arrhenius equation.

 

[kittymaniac84]

Excuse me, why the rude behavior? This is suppose to be a help forum. It might be obvious to you, but I'm not sure if I am using the equation right.

 

[pkleinod]

The Arrhenius equation is ln(k) = ln(A) - E/(RT). You are given values of k at two different temperatures T. R is the gas constant, A and E are empirical constants, E being the activation energy. So just plug the corresponding values (k,T) into this equation to generate two equations in two unknowns. After you know A and E, use the equation to get k at any other T. Does this help?

 

[kittymaniac84]

Yes thank you. I already figured this out on my own. That is exactly what I did. Ea=100,232, A=8.47x10^9, and with T=425 I got 4.06x10^-3 for k.

I hope i did the math right but it looks right.