{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

EXP12 Chemicalreaction rate

EXP12 Chemicalreaction rate - Name Jenny Yoon Partner Adam...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Name: Jenny Yoon Date Performed: 1/29/08Lab Partner: Adam Potts Date Submitted: 2/5/08 Instructor: Xu Zhou Chemical Reaction Rate Objective: To measure the decrease in the concentration of hydrogen peroxide solution as its catalyst is decomposing. To graph the results and find the first order rate constant and the half life of the decomposition rate. Experimental Data: Time (min) Volume of KMnO 4 (mL) 1 6.20 6 5.70 11 5.70 16 5.40 21 4.70 31 3.90 41 3.80 51 3.30 61 3.40 Concentration of KMnO 4 : 0.063 M Sample Calculation 1.Moles of KMnO 4 : Moles = Molarity X Liters 0.063 M X .00620 L = 0.000391 moles KMnO 4 2. Moles of H 2 O 2 : Mole Ratio: 5/2 0.000391 moles KMnO 4 X 5/2 = 0.000978 moles H 2 O 2 3. [H 2 O 2 ] : Molarity = moles / Liters 0.000978 H 2 O 2 / 0.001 L = 0.00978 M H 2 O 2 4. ln[H 2 O 2 ]: 5. 2 2 0 [ ] ln 2 H O : (from graph) ln[H 2 O 2] = -2.31 e -2.31 = 0.0992 0.0992 / 2 = 0.0496 ln(0.0496) = -3.00 6. t 1/2 : y = -0.011x – 2.31 (-3.00) = -0.011x – 2.31 t 1/2 = 62.7 mins 7. k: k = 0.693 / t 1/2 k = 0.693 / 62.7 min k = 0.011 8. [H 2 O 2 ] calc : ln[A] t = ln[A] 0 – kt ln[?] = -2.31 – (0.011)(6) = e -2.37 = 0.0930 M
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Result and Conclusions: Time, min V KMnO4 [H 2 O 2 ] ln[H 2 O 2 ] [H 2 O 2 ] calc 1 6.20 0.00156 -6.46 0.0982 6 5.70 0.00143 -6.55 0.0930 11 5.70 0.00143 -6.55 0.0880 16 5.40 0.00136 -6.60 0.0834 21 4.70 0.000118 -6.74 0.0788 31 3.90 0.000984 -6.92 0.0706 41 3.80
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}