[ninjex]

Hello, I am in need of assistance. I am currently doing my lab report and I am doing the calculations, but something is wrong, or I need clarification.  So background info on the lab. I used  1mL of 0.010 KI, 1mL .001 Na2S2O3 1mL HCL 1mL 1% starch solutipon and then I used 1 mL KBrO3 to mix in all that. I'm supposed to find the reaction rates in respect to temp etc... anyway after experimnentation,  at 283.1 K it required 345 seconds, for a color change, 183 seconds at 293.8 K 73 seconds at 304.3 K and 43 seconds at 314.1 K.  After reading my instructions, the rate = .0010M/the time in seconds. next I need to find my rate constant value. The formula turned out to be [0.0020]^1[0.0080]^1[0.020]^2 or 6.4x10-9. Then I found my k value which is [rate]/[6.4x10-9]. I'm fine up to this point. My trouble begins when I have to graph the ARRHENIUS plot.  I know the slope should be negative, but the k (rate constant) values increase as the temperature increases and the thus the natural log values would increase as well. this would give me a positive slope. What am I doing wrong? When I look up the plot on images,  its always lnk vs inverse temp, so I can't magically make my natural log vaules negative....