Kinetics - experiment Starter…

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Presentation transcript:

Kinetics - experiment Starter… Hydrogen peroxide (H2O2) decomposes in the presence of manganese(IV) dioxide to form water and oxygen gas in a first order manner with respect to H2O2. Write a balanced symbol equation. What method would you use to measure the rate? If the initial concentration of H2O2 was 0.98 mol dm-3 and 20cm3 of O2 was given off. What is the concentration of H2O2 after 20s? Sketch the expected time/conc and conc/rate graphs. Review question maybe using a mind map on a white board

5 week plan single lessons Week 1 – Measuring rates and orders Week 2 – Initial rates method Week 3 – Rate equation Week 4 – Review of papers Week 5 – Rates CPAC If you miss a session you MUST download the PowerPoint from the shared area and collect associated materials, this is your responsibility. You must complete all homeworks or you will not be allowed onto Y13 chemistry. No excuses

Decomposition of H2O2 2H2O2(aq)  2H2O(l) + O2(g) Gas collection method. 2H2O2(aq)  2H2O(l) + O2(g) O2 n = 20cm3 / 24,000 cm3mol-1 O2 n = 0.00083 mol H2O2 n used @ 20s = 0.00083 mol dm-3 x 2 = 0.00167 [H2O2] used @ 20s = (0.00167/5cm3) x1000 = 0.334 mol dm-3 [H2O2]ini - [H2O2]used @ 20s = 0.98 – 0.334 = 0.646 mol dm-3

Task Your task is to confirm that the reaction is first order with respect to H2O2 by using one of two methods. Method 1 Set up the experiment as shown by your teacher. Place 5cm3 of 0.98M H2O2 into the flask and connect the collection hose. Add a small amount of MnO2 catalyst ensuring that the stopper is replaced quickly. Time how long it takes for 40cm3 of O2 to be collected. Repeat with 1.96M, 2.94M and 3.96M Method 2 Set up the experiment as shown by your teacher. Place 5cm3 of 1.96M H2O2 into the flask and connect the collection hose. Add a small amount of MnO2 catalyst ensuring that the stopper is replaced quickly. Record the volume of O2 every 10s until 40cm3 is collected Repeat 2x more.

Tables Your task is to confirm that the reaction is first order with respect to H2O2 by using one of two methods. Method 2 Method 1 Time (s) vol O2 (cm3) [H2O2] (mol dm-3) Rate ([H2O2] s-1) 10 20 30 40 50 [H2O2] (mol dm-3) Time (s) rate (s-1) 0.98 1.96 2.94 3.92

Processing Use the excel file to process your results. Method 1 Plot a graph of time vs concentration. Use the half life method to calculate the order. Calculate 1/t to get the rate. Plot concentration vs rate. Use the shape to determine the order. Method 2 Plot a graph of time vs concentration. Use the half life method to calculate the order. Calculate the gradient every 10 seconds Plot concentration vs rate. Use the shape to determine the order.