chemical reaction rate

chemical reaction rate - Date Performed: 2/2/06 Date...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Date Performed: 2/2/06 Name: Ronald Lampkins Date Submitted: 2/9/06 Partner: Jason Herrala Instructor: Shengliang Zhao Chemical Reaction Rate Objectives: To measure the decrease in the concentration of a hydrogen peroxide solution as it is catalytically decomposing. To graph the results and form the graph deduce the first order reaction rate constant and the half-life of the decomposition reaction. Experimental Data: Time (min) KMnO4 9 (mL) 1 6.61 6 4.89 11 4.15 16 3.80 21 3.40 31 3.15 41 2.65 51 1.20 61 0.83 Initial molarity of potassium permanganate solution: 0.063 M Sample Calculations: 1. Moles of KMnO 4 Time 1 0.063 M KMnO 4 = x / .00661 L X = 4.16 x 10 -4 moles KMnO 4 2. Moles of H 2 O 2 Time 1 5/2 x moles KMnO 4 5/2 x 4.16 x 10 -4 moles KMnO 4 = 1.0 x 10 -3 moles H 2 O 2 3. Molarity of H 2 O 2 Time 1 M = mol / L 0.001 mol H 2 O 2 / .01 mL H 2 O 2 = 1.0 x 10 -1 M H 2 O 2
Background image of page 1

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

View Full DocumentRight Arrow Icon
4. ln[A] 0 = -2.33 e^2.33 = 0.097 0.097 / 2 = 0.048 ln 0.048 = -3 -3 on the y-intercept crosses at 22 minutes Half-life = 22 min
Background image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 2

chemical reaction rate - Date Performed: 2/2/06 Date...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online