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Question

The rate of constant for the reaction Br(g) + O₃(g) —> BrO(g) + O₂(g) was determined at the four temperatures shown below.

T (K): k[cm³/molecules•s):

238 5.90 x 10^-13

258 7.70 x 10^-13

278 9.60 x 10^-13

298 1.20 x 10^-12

The value of R = 8.314 (J/mol•K).

^{Plot the above data, and then use that data to calculate the activation energy for this reaction.}

^{____ J}

^{Can someone please help me answer this}

Answer 1

I can help you answer this, but I can't draw the graph on this platform, so you'll have to do it. If you want to understand more about this process, look up and read about the Arrhenius equation and the Arrhenius plot.

In this problem, you'll use the Arrhenius plot where you plot ln k on the y-axis versus 1/T on the x-axis. You should get a straight line with a negative slope. The equation for this line is...

ln k = -Ea/R (1/T) = ln A and this is in the form y = mx + b (straight line)

The slope of the line = -Ea/R so just divide the slope by 8.314 J/mol-K to obtain the value of -Ea or divide it by 0.008314 kJ/K-mol to get the answer is kJ/mol which is the more common unit for Ea.