November+22nd+Class+Lab+Results

The formula to calculate rate of reaction is Change in concentration/elapsed time but the calculations most people are using is the calculations to find order of reaction. Page 360 in the chem. textbook confirms the equation.

Reaction: The decomposition of hydrogen peroxide
 * Investigation 6.2.1 - Roseanne, Vinod, Brittany**

The rates of reaction were attained by calculating the slope of the volume vs. time graph The rate of reaction for each of the three separate trials were as follows:

1.22 mL·s-1 at 30˚C 2.42 mL·s-1 at 50˚C 3.87 mL·s-1 at 70˚C

The purpose of our investigation was to see how change in temperature affects the rate of reaction. Amount of calcium chloride and volume of hydrogen peroxide were kept constant. CaCO3(s) + 2HCl → CaCl2 (aq) + H2O (g) + CO2 (g) g) As time increases, the [HCl] decreases and therefore pH of the solution increases; becoming more basic. Also rate of reaction decreases as time increases.
 * Investigation 6.2.1 - Melissa, Aditi, Patricia, Shama**
 * Mathematically:**
 * Finding the rate of reaction: Temperature 23 oC**

0.0630957 a) ↓ 0.0398107
 * [H2O2] (mol/L)**

r is proportional to 1 /∆t r=1/8= 0.125s-1 b) ↓ r 1/12 0.0833 s-1 a) Change factor for [H2O2]: 0.0630957 / 0.0398107 = 1.585 b) Change factor for rate of reaction: 0.125 s-1/ 0.0833 s-1 = 1.5006 (1.585)^m =1.5006 m = log 1.5006 / log 1.585 m =0.88 r = k[H2O2]^0.88
 * Rate of reaction**

0.0501187 a) ↓ 0.0125893 r= 1/8 = 0.125 s-1 b) ↓ r= 1/12 = 0.0833 s-1 a) Change factor for [H2O2]: 0.0501187/0.0125893 = 3.983 b) Change factor for rate of reaction: 0.125 s-1/ 0.0833 s-1 = 1.5006 (3.983)^ m = (1.5006) m = log 1.5006 / log3.983 m= 0.294
 * Temperature 40 oC**
 * [H2O2] (mol/L)**
 * Rate of reaction:**

0.00158489 a) ↓ 2.51189e^-05 r= 1/8=0.125 s-1 b) ↓ r= 1/12 = 0.0833 s-1 a) Change factor for [H2O2]: 0.00158489/2.51189e^-05 = 0.093642051 b) Change factor for rate of reaction: 0.125 s-1/ 0.0833 s-1 = 1.5006 (0.09364)^ m = (1.5006) m = log 1.5006 / log 0.09364 m= -0.17
 * Temperature 60 oC**
 * [H2O2] (mol/L)**
 * Rate of reaction:**


 * Investigation 6.2.1 - Bardia, Wendy, Peter**

We performed the experiment: metals reacting with acids. We used the zinc metal. Exp.1: (0.19952623 - 0.063095734)/(4-0) =-1.108mol/(L.min) Experiment 2: r is proportional to 1/t (0.316227766 -0.501187234)/(4-0) =-0.0462mol/(L.min)
 * Investigation 6.2.1 - Funmbi, Heather, Vani**

was designed to observe the change in rate of reaction depending on the heat of the environment that the reaction took place in.
 * Chris, Karl, Jen and Natalie (I hope this is the right group, sorry, I accidentally deleted your names).



As is obvious by looking at our results, there is no patern whatsoever in the results we collected. This is because our pH meter wasn't working properly. In an acidic solution, it would not stay stable, and would fluctuate anywhere from 0.0 to 3.0 pH. We therefore cannot draw any conclusions from our data.**